{"id":1817,"date":"2022-06-26T18:26:50","date_gmt":"2022-06-26T18:26:50","guid":{"rendered":"https:\/\/blog.praxilabs.com\/?p=1817"},"modified":"2025-10-19T17:41:51","modified_gmt":"2025-10-19T17:41:51","slug":"9-vital-chemistry-laws-and-formulas","status":"publish","type":"post","link":"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/","title":{"rendered":"9 Essential Chemistry Laws and Formulas You Should Know!"},"content":{"rendered":"<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Chemistry is the branch of science through which interactions and reactions between different atoms, electrons, elements, molecules, and many other particles are being analyzed, tested, and studied.<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">As a vital branch of science, chemistry exists around us in a daily manner, whereas chemical interactions and reactions do not occur haphazardly; rather they are all governed by many chemistry laws that our scientists managed to figure out many years ago for our human civilization.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">And whether you<span style=\"font-weight: 400;\"> are a science student or not, it is necessary to\u2014at least\u2014be familiar with the most important chemistry laws that govern this science, understand their nature, and maybe study them <\/span><span style=\"font-weight: 400;\">as essential chemistry knowledge.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In this article, we cover the <\/span><b>9<\/b><span style=\"font-weight: 400;\"> most critical chemistry laws and how they work\u2026 Let\u2019s start!<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 12pt;\"><a class=\"maxbutton-3 maxbutton\" href=\"https:\/\/praxilabs.com\/\"><span class='mb-text'>Get started Praxilabs for FREE<\/span><\/a><\/span><\/strong><\/span><\/p>\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_83 counter-hierarchy ez-toc-counter ez-toc-light-blue ez-toc-container-direction\">\r\n<div class=\"ez-toc-title-container\">\r\n<p class=\"ez-toc-title\" style=\"cursor:inherit\">Table of Contents<\/p>\r\n<span class=\"ez-toc-title-toggle\"><\/span><\/div>\r\n<nav><ul class='ez-toc-list ez-toc-list-level-1 ' ><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#_Chemistry_Laws_The_Fundamental_Chemistry_Principles\" >\u00a0Chemistry Laws | The Fundamental Chemistry Principles<\/a><ul class='ez-toc-list-level-3' ><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#The_law_of_conservation_of_mass\" >The law of conservation of mass<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#The_law_of_constant_proportions\" >The law of constant proportions<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#The_law_of_multiple_proportions\" >The law of multiple proportions<\/a><\/li><\/ul><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Chemical_Formulas\" >Chemical Formulas<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-6\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Learn_More_About_General_Chemistry\" >Learn More About General Chemistry<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-7\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Organic_Chemistry_Laws\" >Organic Chemistry Laws<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-8\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#5_Live-Changing_Laws_of_Chemistry\" >5 Live-Changing Laws of Chemistry<\/a><ul class='ez-toc-list-level-3' ><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-9\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Avogadros_Law\" >Avogadro\u2019s Law<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-10\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Boyles_Law\" >Boyle\u2019s Law<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-11\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Boyles_law_practice_problems\" >Boyle\u2019s law practice problems<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-12\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Charles_Law\" >Charles\u2019 Law<\/a><\/li><\/ul><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-13\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Boyles_law_vs_Charless_law\" >Boyle\u2019s law vs. Charles\u2019s law<\/a><ul class='ez-toc-list-level-3' ><li class='ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-14\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Gay-Lussacs_Law\" >Gay-Lussac\u2019s Law<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-3'><a class=\"ez-toc-link ez-toc-heading-15\" href=\"https:\/\/praxilabs.com\/en\/blog\/2022\/06\/26\/9-vital-chemistry-laws-and-formulas\/#Ideal_Gas_Law\" >Ideal Gas Law<\/a><\/li><\/ul><\/li><\/ul><\/nav><\/div>\r\n<h2><span class=\"ez-toc-section\" id=\"_Chemistry_Laws_The_Fundamental_Chemistry_Principles\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">\u00a0<\/span><b>Chemistry Laws <\/b><b>| The Fundamental Chemistry Principles<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Chemistry laws are many, and they are subject to changing and evolving with every new detection and discovery. These laws work hand in hand with every other law that we know rules other phenomena and reactions. Whether these laws are biological, mathematical, or physical, they are all still seen as \u201cthe laws of nature.\u201d<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">In chemistry, three laws are looked at as the \u201cfundamental chemistry principles\u201d which govern the behavior of matter.<\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">These 3 basic chemistry concepts are:<\/span><\/p>\n<ol>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The law of conservation of mass.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The law of constant proportions.<\/span><\/li>\n<li style=\"font-weight: 400;\" aria-level=\"1\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The law of multiple proportions.<\/span><\/li>\n<\/ol>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Throughout your chemistry studies, you may have worked closely with these laws, without necessarily knowing their true nomenclature. Here, we will discuss each one of them in detail.<\/span><\/span><\/p>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"The_law_of_conservation_of_mass\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>The law of conservation of mass<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b><\/b><span style=\"font-weight: 400;\">The law of conservation of mass law dates back to Antoine-Laurent de Lavoisier\u2019s discovery in 1789, stating the fact that:<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">&#8220;mass is neither created nor destroyed in chemical reactions.&#8221;<\/span><\/i><\/span><\/p>\n<p style=\"text-align: left;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In other words, and for a <\/span><b>closed system,<\/b><span style=\"font-weight: 400;\"> the total mass of both the reactants and the products of a chemical reaction will remain the same throughout that reaction and at any point in time during that reaction.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">This discovery was proven true with calculations and experiments, bearing in mind that almost all naturally formulated elements are very stable given the conditions of our Earth\u2019s surface. By this, the foundation for modern chemistry was laid.<\/span><\/p>\n<figure id=\"attachment_1821\" aria-describedby=\"caption-attachment-1821\" style=\"width: 300px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\"size-medium wp-image-1821\" src=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/law-of-conservation-of-mass_combustion-reaction-of-methane-300x134.jpg\" alt=\"law of conservation of mass\" width=\"300\" height=\"134\" srcset=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/law-of-conservation-of-mass_combustion-reaction-of-methane-300x134.jpg 300w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/law-of-conservation-of-mass_combustion-reaction-of-methane-768x343.jpg 768w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/law-of-conservation-of-mass_combustion-reaction-of-methane.jpg 1009w\" sizes=\"auto, (max-width: 300px) 100vw, 300px\" \/><figcaption id=\"caption-attachment-1821\" class=\"wp-caption-text\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">An illustration for the combustion of methane as an example of the law of conservation of mass (Source: <a href=\"https:\/\/en.wikipedia.org\/wiki\/Conservation_of_mass\" target=\"_blank\" rel=\"noopener\">Wikipedia<\/a>)<\/span><\/figcaption><\/figure>\n<ul>\n<li style=\"font-weight: 400;\" aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"The_law_of_constant_proportions\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>The law of constant proportions<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b><\/b><span style=\"font-weight: 400;\">Also known as \u201cthe law of <\/span><i><span style=\"font-weight: 400;\">definite<\/span><\/i><span style=\"font-weight: 400;\"> proportions\u201d or \u201cProust\u2019s law\u201d, it was first stated by the French chemist Louis Proust in 1779, based on his work on sulfides, metallic oxides, and sulfates. Yet, the first observations referring to this law were made by both the chemists Antoine Lavoisier and Joseph Priestley.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The law states that:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">&#8220;Individual elements constituting a particular chemical compound are present in a <\/span><\/i><b><i>fixed <\/i><\/b><i><span style=\"font-weight: 400;\">ratio (in terms of their mass), regardless of their source.&#8221;<\/span><\/i><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">For better comprehension, a pure water molecule will always consist of <\/span><b>two <\/b><span style=\"font-weight: 400;\">hydrogen atoms and <\/span><b>one<\/b><span style=\"font-weight: 400;\"> oxygen atom, forming the well-known <\/span><b>2:1 ratio.<\/b><span style=\"font-weight: 400;\"> A gram of pure water\u2014in case you are into numbers\u2014approximately includes 0.11 grams of hydrogen and 0.88 grams of oxygen.<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Another example of a famous chemical compound obeying this law is <\/span><b>methane. <\/b><span style=\"font-weight: 400;\">It takes <\/span><b>four <\/b><span style=\"font-weight: 400;\">hydrogen atoms and <\/span><b>one <\/b><span style=\"font-weight: 400;\">carbon atom to successfully bring out <\/span><b>one<\/b><span style=\"font-weight: 400;\"> methane molecule.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">An exception to this law is <\/span><b>non-stoichiometric<\/b><span style=\"font-weight: 400;\"> compounds, where the elements\u2019 ratio varies from one sample to another. Also the samples of elements that vary in their <\/span><b>isotopic <\/b><span style=\"font-weight: 400;\">composition and natural polymers are both known to defy and disobey this law.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In a nitrogen dioxide (NO<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">) molecule, the ratio of the number of nitrogen and oxygen atoms is <\/span><b>1:2,<\/b><span style=\"font-weight: 400;\"> and its mass ratio is 14:32 (or 7:16). Hence, it <\/span><b>does not obey <\/b><span style=\"font-weight: 400;\">the law of constant proportions.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">This law was not met by open arms amongst the scientific community in the beginning, rather, with much opposition. It was not until Dalton\u2019s atomic theory that this law was favored. A relation between <\/span><a href=\"https:\/\/byjus.com\/chemistry\/law-constant-proportion\/\" target=\"_blank\" rel=\"nofollow noopener\"><span style=\"font-weight: 400;\">the theory and the law<\/span><\/a><span style=\"font-weight: 400;\"> was established in 1811 by the Swedish chemist Jacob Berzelius, only then was it accepted.<\/span><b><\/b><\/span><\/p>\n<ul>\n<li aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"The_law_of_multiple_proportions\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>The law of multiple proportions<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">As a consequence of the idea of combining elements to form compounds, introduced by known as <\/span><b>\u201cDalton\u2019s Law,\u201d <\/b><span style=\"font-weight: 400;\">was proposed in 1804 by the English meteorologist John Dalton. The law states that:<\/span><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">&#8220;When elements combine and form compounds, the proportions of those primary elements can be expressed in a ratio of small whole numbers.&#8221;<\/span><\/i><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">An example is the reaction of carbon and oxygen that can lead to the formation of both carbon monoxide (CO) and carbon dioxide (CO<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">). In CO, the ratio of the oxygen amount to that of carbon is 1:1, while in CO<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">, the ratio is 1:2, and both are ratios of simple whole numbers.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">This law is one cornerstone of the recognized modern atomic theory and comes side by side with the laws of mass conservation and the law of definite proportions. All together, these laws reinforce Dalton\u2019s assumption and concept which acknowledge matter to be composed of different indivisible combinations of some building blocks of matter, i.e., atoms.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Our current understanding of atomic composition and structure was based on these laws and theories, not to forget including other vital concepts such as molecular, or chemical formulas.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Chemical_Formulas\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Chemical Formulas<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The human\u2019s chemical literacy is incubated by his\/her ability to form and include a simple common language which easily expresses and represents a compound, a molecule, or even a single element. All of these come in contact together in order to express a series of reactions and interactions throughout some letters and numbers.<\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">This <\/span><b>common <\/b><span style=\"font-weight: 400;\">language is\u00a0 hence called <\/span><b>a chemical formula. <\/b><span style=\"font-weight: 400;\">And it is defined as follows:<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><\/i><i><span style=\"font-weight: 400;\">&#8220;An expression of chemical symbols and numerical subscripts that represents the composition of one unit of a compound.&#8221;<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Be careful not to confuse the definition and usage of a \u201cchemical formula\u201d with that of a \u201cstructural formula,\u201d where the latter is a 2D graphical representation showing the atoms&#8217; spatial relationships that form the molecule or the compound.<\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Chemical formulas depend entirely on the compound\u2019s number of consistent atoms and their ratios shown in numbers. These formulas can be simple, i.e., H (referring to hydrogen), or complex, as is the case with CH<\/span><sub><span style=\"font-weight: 400;\">3<\/span><\/sub><span style=\"font-weight: 400;\">CH<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">OH (referring to ethanol).<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It is very necessary for you\u2014if you are a clever student or a scientist\u2014to wholeheartedly know and memorize as many chemical formulas as you can.<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 12pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong><a class=\"maxbutton-3 maxbutton\" href=\"https:\/\/praxilabs.com\/en\/pricing\"><span class='mb-text'>Book FREE Live Demo Now<\/span><\/a>\u00a0<\/strong><\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Learn_More_About_General_Chemistry\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Learn More About General Chemistry<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">General chemistry is a branch of chemistry that focuses on studying matter, energy, and the interactions between them. It serves as a broad introduction to various concepts and basics in chemistry. It is often taught in high school chemistry courses, as well as at the introductory university levels.\u00a0<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">General chemistry covers a wide range of topics, including:<\/span><\/p>\n<ul>\n<li><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Conservation of mass.<\/span><\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Elementary atomic theory.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Periodic table and periodicity.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Acid-base chemistry.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Law of constant composition.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Law of gases.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Nuclear chemistry.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Solubility.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Chemical bonding.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Chemical kinetics.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Thermodynamics.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Electrochemistry.<\/span><\/li>\n<li><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Chemical equilibria.<\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">These topics are essential for understanding many aspects of the natural world and various applications of chemistry.<\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"Organic_Chemistry_Laws\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Organic Chemistry Laws<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">There is a dedicated branch of chemistry that is devotedly concerned with studying and understanding\u2014but not memorizing\u2014organic compounds<\/span><span style=\"font-weight: 400;\">\u00a0and all the interactions and relations between them.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Organic chemistry requires passionate students that are truly fond of chemistry, in order to grasp and maintain all its laws and compounds\u2019 nomenclature. This exciting branch is ruled by many of the \u201cregular\u201d chemistry laws, as well as other exclusive ones that are tailored to adhere to its eccentricity.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Aside from learning the basics, organic chemistry can fit well under the umbrella of its <\/span><b>\u201cgolden rules.\u201d <\/b><span style=\"font-weight: 400;\">Compost, organic fuel, alcohol, urea, and acetone are forms of organic compounds existing in our day-to-day lives.<\/span><\/span><\/p>\n<h2><span class=\"ez-toc-section\" id=\"5_Live-Changing_Laws_of_Chemistry\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>5 Live-Changing Laws of Chemistry<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Since science is a revolutionizing human-invented tool, it is constantly developing, and its remarkable steps were\u2014and still are\u2014achieved by connecting the dots of all the laws and pieces of information all together, and bingo! A new law, observation, or device is formulated, discovered, or invented.<\/span><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">In this section, <\/span><b>5 <\/b><span style=\"font-weight: 400;\">gas-related live-changing chemistry laws will be explained and discussed. These laws mainly deal with temperature, pressure, volume, and many other characteristics that control how atoms, elements, and compounds behave in different conditions. The laws are:<\/span><\/span><\/p>\n<ul>\n<li aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"Avogadros_Law\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Avogadro\u2019s Law<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">If you studied chemistry only as an introductory course, you would have probably dealt with Avogadro\u2019s law. This famous law states that:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cEqual volumes of all gasses, at the same temperature and pressure, have the same number of molecules.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Hypothesized in 1811, this empirical law was named after Amedeo Avogadro, a higher physics professor at the University of Turin. Nevertheless, his law was not accepted among the scientific society until after 1958, when a logical chemical system, constructed by the Italian chemist Stanislao Cannizzaro, was entirely based on it.<\/span><\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"wp-image-4635 size-medium aligncenter\" src=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/07\/Essential-Chemistry-Laws-and-Formulas-3-231x300.webp\" alt=\"Scientist Amedeo Avogadro\" width=\"231\" height=\"300\" srcset=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/07\/Essential-Chemistry-Laws-and-Formulas-3-231x300.webp 231w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2025\/07\/Essential-Chemistry-Laws-and-Formulas-3.webp 768w\" sizes=\"auto, (max-width: 231px) 100vw, 231px\" \/><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Amedeo proposed that <\/span><b>ideal gasses<\/b><span style=\"font-weight: 400;\"> at the same volume, and in the same conditions of temperature and pressure, contain an equal number of molecules! This certain number of molecules is scientifically denoted as <\/span><b>Avogadro\u2019s number, <\/b><span style=\"font-weight: 400;\">and it is equal to <\/span><b>6.02214076 x 10<\/b><b>23<\/b><b> molecules.<\/b><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Its mathematical representation is defined as<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">V \u03b1 n, or<\/span><\/strong><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">V\/n = \u03ba<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">where<\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>V:<\/b><span style=\"font-weight: 400;\"> the volume of the gas<br \/>\n<\/span><b>n:<\/b><span style=\"font-weight: 400;\"> the amount of substance of the gas (measured in moles)<br \/>\n<\/span><b>k:<\/b><span style=\"font-weight: 400;\"> a constant for a given temperature and pressure<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Under two sets of conditions, the relation between same compounds and substances is expressed as<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">V<\/span><sub><span style=\"font-weight: 400;\">1<\/span><\/sub><span style=\"font-weight: 400;\">\/n<\/span><sub><span style=\"font-weight: 400;\">1<\/span><\/sub><span style=\"font-weight: 400;\">=<\/span><span style=\"font-weight: 400;\">V<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">\/n<\/span><sub><span style=\"font-weight: 400;\">2<\/span><\/sub><span style=\"font-weight: 400;\">.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">This equation defines a relation between the number of moles of the gas and the volume of it, where it forms a direct proportion ratio.<\/span><\/p>\n<ul>\n<li aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"Boyles_Law\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Boyle\u2019s Law<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cAt constant temperature, the pressure exerted by a given quantity of gas varies inversely with the volume occupied by it.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Boyle\u2019s law<\/span><span style=\"font-weight: 400;\"> is another empirical relation that describes and discusses gasses\u2019 compression and expansion. This law was formulated in 1662 by the physicist Robert Boyle, where its mathematical equation is given by<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">p \u03b1 1\/V, or<\/span><\/strong><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">pV = K<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">where<\/span><\/p>\n<ul>\n<li><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>P: <\/b><span style=\"font-weight: 400;\">the pressure exerted by the gas.<br \/>\n<\/span><b>V: <\/b><span style=\"font-weight: 400;\">the volume occupied by the gas.<br \/>\n<\/span><b>K: <\/b><span style=\"font-weight: 400;\">proportionality constant.<\/span><\/span><\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">If the gas is put in a container and a work is done on it, or by it, the following relation can be used to determine the pressure value:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">p<sub>1<\/sub>V<sub>1 <\/sub>= p<sub>2<\/sub>V<sub>2<\/sub>.<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The law is functionally used in many applications and some of them are mentioned in this interesting article: <\/span><span style=\"font-weight: 400;\">3 of the Most Important Applications of <\/span><a href=\"https:\/\/praxilabs.com\/en\/blog\/2019\/05\/16\/applications-of-boyles-law-en\/\"><span style=\"font-weight: 400;\">Boyle\u2019s Law<\/span><\/a><span style=\"font-weight: 400;\">.\u201d<\/span><\/span><\/p>\n<h3><span class=\"ez-toc-section\" id=\"Boyles_law_practice_problems\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Boyle\u2019s law practice problems<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<ol>\n<li><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b> A gas occupies 12.3 liters at a pressure of 40.0 mm Hg. What is the volume when the pressure is increased to 60.0 mm Hg?<\/b><\/span><\/li>\n<\/ol>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">To solve this problem, we can use Boyle&#8217;s law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">According to Boyle&#8217;s law, we can set up the following equation:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">P1V1 = P2V2<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Plugging in the given values:<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">(40.0 mm Hg) (12.3 L) = (60.0 mm Hg) (V2)<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Simplifying the equation:<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">492 L mm Hg = 60.0 mm Hg V2<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Dividing both sides by 60.0 mm Hg:<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">V2 = 8.2 L<\/span><\/p>\n<ol start=\"2\">\n<li><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b> A gas occupies 1.56 L at 1.00 atm. What will be the volume of this gas if the pressure increases to 3.00 atm?<\/b><\/span><\/li>\n<\/ol>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">To solve this problem, we can use Boyle&#8217;s law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">According to Boyle&#8217;s law, we can set up the following equation:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">P1V1 = P2V2<\/span><\/strong><\/span><\/p>\n<ul>\n<li style=\"text-align: left;\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Plugging in the given values:<\/span><\/li>\n<\/ul>\n<p style=\"text-align: left;\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">(1 atm) (1.56 L) = (3 atm)(V2)<\/span><\/p>\n<ul>\n<li style=\"text-align: left;\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Simplifying the equation:<\/span><\/li>\n<\/ul>\n<p style=\"text-align: left;\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">1.56 L atm = 3 atm V2<\/span><\/p>\n<ul>\n<li style=\"text-align: left;\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Dividing both sides by 3 atm:<\/span><\/li>\n<\/ul>\n<p style=\"text-align: left;\"><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">V2 = 0.52 L<\/span><\/p>\n<ul>\n<li aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"Charles_Law\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Charles\u2019 Law<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">In his unpublished work from the 1780s, the scientist Jacques Charles formulated this law, which is also known as \u201cthe law of volumes\u201d.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The law states that:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cThe volume occupied by a fixed amount of gas is directly proportional to its absolute temperature, if the pressure remains constant.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Frankly speaking, this law describes how gasses favor to expand when they are heated.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The mathematical equation is given by<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">V \u03b1 T, or<\/span><\/strong><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><strong>VT = K.<\/strong><span style=\"font-weight: 400;\"><br \/>\n<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">If a comparison is obtained, we can use the following formula:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">V<sub>1<\/sub>\/T<sub>1 <\/sub>= V<sub>2<\/sub>\/T<sub>2<\/sub>.<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">From these equations we deduce that an inverse relation exists between the temperature and the volume.<\/span><\/p>\n<figure id=\"attachment_1820\" aria-describedby=\"caption-attachment-1820\" style=\"width: 351px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" class=\" wp-image-1820\" src=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/charles-law-in-chemistry-1-300x165.png\" alt=\"Charles' law illustrated\" width=\"351\" height=\"193\" srcset=\"https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/charles-law-in-chemistry-1-300x165.png 300w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/charles-law-in-chemistry-1-768x423.png 768w, https:\/\/praxilabs.com\/en\/blog\/wp-content\/uploads\/2022\/06\/charles-law-in-chemistry-1.png 819w\" sizes=\"auto, (max-width: 351px) 100vw, 351px\" \/><figcaption id=\"caption-attachment-1820\" class=\"wp-caption-text\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">An illustration explaining Charles&#8217; law (Source: <a href=\"https:\/\/letstalkscience.ca\/educational-resources\/backgrounders\/charles-law-and-gay-lussacs-law\" target=\"_blank\" rel=\"noopener\">Let&#8217;s Talk Science<\/a>)<\/span><\/figcaption><\/figure>\n<h2><span class=\"ez-toc-section\" id=\"Boyles_law_vs_Charless_law\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Boyle\u2019s law vs. Charles\u2019s law<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h2>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Boyle&#8217;s law and Charles&#8217;s law are two fundamental gas laws that describe the relationship between different properties of gasses. Let\u2019s differentiate between them:<\/span><\/p>\n<table>\n<tbody>\n<tr>\n<td>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Boyle\u2019s Law\u00a0<\/b><\/span><\/p>\n<\/td>\n<td>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Charles&#8217;s Law<\/b><\/span><\/p>\n<\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It states that at a constant temperature, the pressure exerted by a given quantity of gas varies inversely with the volume it occupies.<\/span><\/td>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It states that the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature if the pressure remains constant.<\/span><\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It gives a relation between the volume and the pressure of the gas.<\/span><\/td>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It gives a relation between the volume and the temperature of the gas.<\/span><\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Mathematically, Boyle&#8217;s law can be expressed as: P1V1 = P2V2<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">\u00a0Where:\u00a0<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">P \u2014&#8212;- pressure\u00a0<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">V \u2014&#8212;- volume<\/span><\/td>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Mathematically, Charles&#8217;s law can be expressed as: V1\/T1 = V2\/T2<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">\u00a0Where:<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">\u00a0V \u2014&#8212;&#8212; volume\u00a0<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">T \u2014&#8212;&#8212;-temperature<\/span><\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The product of the pressure and the volume is constant (PV = k).<\/span><\/td>\n<td><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>T<\/b><span style=\"font-weight: 400;\">he temperature and volume ratio is constant (V = kT).<\/span><\/span><\/td>\n<\/tr>\n<tr>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It is often applied to situations involving changes in the volume of a gas, such as compressing or expanding a gas in a container.<\/span><\/td>\n<td><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It is often applied to situations involving changes in the volume of a gas due to changes in temperature, such as heating or cooling a gas in a container.<\/span><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<ul>\n<li aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"Gay-Lussacs_Law\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Gay-Lussac\u2019s Law<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Formulated in 1808 by the French chemist Joseph Gay-Lussac, this law is another important cornerstone in gas laws. It states that:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cBoth the pressure and the temperature of an ideal gas are directly proportional, assuming constant mass and volume.\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The mathematical expression of the law can be written as<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">P \u03b1 T, or<\/span><\/strong><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">P\/T = K.<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Note that <\/span><b>T <\/b><span style=\"font-weight: 400;\">is the <\/span><b>absolute <\/b><span style=\"font-weight: 400;\">temperature of the gas and not any haphazard temperature.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Gay-Lussac\u2019s effect is tangible in our everyday\u2019s life. Examples can vary from noticing your car tires\u2019 pressure in winter as it drops to keeping an eye on your propane tanks at home. The tires and the propane tanks read higher or lower pressure upon the temperature surrounding them.<\/span><\/p>\n<ul>\n<li aria-level=\"1\">\n<h3><span class=\"ez-toc-section\" id=\"Ideal_Gas_Law\"><\/span><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>Ideal Gas Law<\/b><\/span><span class=\"ez-toc-section-end\"><\/span><\/h3>\n<\/li>\n<\/ul>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">It&#8217;s also known as \u201cthe general gas equation.\u201d And although this law has some limitations, it stands as a good approximation of gasses\u2019 behavior in many different conditions.\u00a0<\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">The law was formulated in 1834 by Beno\u00eet Paul \u00c9mile Clapeyron\u00a0<\/span><span style=\"font-weight: 400;\">and represents a combination of all the previously mentioned ones, i.e., Avogadro\u2019s, Boyle\u2019s, Charles\u2019s, and Gay-Lussac\u2019s.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">The law states that:<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><i><span style=\"font-weight: 400;\">\u201cFor a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature,\u201d<\/span><\/i><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">where this is mathematically expressed as<\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 14pt;\">pV = nRT,<\/span><\/strong><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">where<\/span><\/p>\n<ul>\n<li><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><b>n: <\/b><span style=\"font-weight: 400;\">the number of the moles of the gas.<br \/>\n<\/span><b>R: <\/b><span style=\"font-weight: 400;\">the ideal gas constant.<\/span><\/span><\/li>\n<\/ul>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Before starting your calculations, make sure that the temperature (T) in use is given in <\/span><b>Kelvins. <\/b><span style=\"font-weight: 400;\">And that <\/span><span style=\"font-weight: 400;\">R=8.3145<\/span><span style=\"font-weight: 400;\"> J.K<\/span><sup><span style=\"font-weight: 400;\">-1<\/span><\/sup><span style=\"font-weight: 400;\">.mol<\/span><sup><span style=\"font-weight: 400;\">-1<\/span><\/sup><span style=\"font-weight: 400;\">, or m<\/span><sup><span style=\"font-weight: 400;\">3<\/span><\/sup><span style=\"font-weight: 400;\">\u22c5Pa\u22c5K<\/span><sup><span style=\"font-weight: 400;\">-1<\/span><\/sup><span style=\"font-weight: 400;\">\u22c5mol<\/span><sup><span style=\"font-weight: 400;\">-1<\/span><\/sup><span style=\"font-weight: 400;\">.<\/span><\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">All in all, simplicity in this relation encourages us to treat gasses as ideal, unless there is a good reason to do otherwise.<\/span><\/p>\n<p><span style=\"font-weight: 400; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\">Chemistry, especially organic chemistry, is an ever-evolving science, and it underlies many key laws and rules that steer everything in our lives. Other chemistry laws, such as Faraday\u2019s law, Graham\u2019s law, and Henry\u2019s law,\u00a0 are all pivotal and fit perfectly in their places.<\/span><\/p>\n<p><span style=\"font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><span style=\"font-weight: 400;\">Many names and laws keep appearing when we maneuver from a state to another and from a condition to another. More experiments await you on <\/span>PraxiLabs \u2014for FREE<span style=\"font-weight: 400;\">\u2014if you are seeking more <a href=\"https:\/\/praxilabs.com\/en\/3d-science-simulations\">3D science experiments<\/a> particularly concerned with chemistry laws or <a href=\"https:\/\/praxilabs.com\/en\/virtual-chemistry-lab\">virtual chemistry lab<\/a>s in general.<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><iframe loading=\"lazy\" src=\"\/\/www.youtube.com\/embed\/GiCnieeoPs0?t=197s\" width=\"560\" height=\"314\" allowfullscreen=\"allowfullscreen\"><\/iframe><\/p>\n<p style=\"text-align: center;\"><span style=\"text-decoration: underline; font-size: 14pt; font-family: tahoma, arial, helvetica, sans-serif;\"><a href=\"https:\/\/praxilabs.com\/\"><b>Sign Up to <span style=\"text-decoration: underline;\">PraxiLabs<\/span> and Start Your <\/b><span style=\"text-decoration: underline;\"><b>FREE<\/b><\/span><b> Virtual Lab Simulation!<\/b><\/a><\/span><\/p>\n<p style=\"text-align: center;\"><span style=\"font-family: tahoma, arial, helvetica, sans-serif;\"><strong><span style=\"font-size: 12pt;\"><a class=\"maxbutton-3 maxbutton\" href=\"https:\/\/praxilabs.com\/en\/virtual-labs\"><span class='mb-text'>Join Us Now for FREE<\/span><\/a><\/span><\/strong><\/span><\/p>\n","protected":false},"excerpt":{"rendered":"<p>Chemistry is the branch of science through which interactions and reactions between different atoms, electrons, elements, molecules, and many other particles are being analyzed, tested, and studied. As a vital branch of science, chemistry exists around us in a daily manner, whereas chemical interactions and reactions do not occur haphazardly; rather they are all governed &hellip;<\/p>\n","protected":false},"author":11,"featured_media":4481,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_lmt_disableupdate":"no","_lmt_disable":"no","footnotes":""},"categories":[3],"tags":[],"class_list":["post-1817","post","type-post","status-publish","format-standard","has-post-thumbnail","","category-chemistry"],"modified_by":"Muhamed Elmesery","_links":{"self":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts\/1817","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/users\/11"}],"replies":[{"embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/comments?post=1817"}],"version-history":[{"count":22,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts\/1817\/revisions"}],"predecessor-version":[{"id":5433,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/posts\/1817\/revisions\/5433"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/media\/4481"}],"wp:attachment":[{"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/media?parent=1817"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/categories?post=1817"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/praxilabs.com\/en\/blog\/wp-json\/wp\/v2\/tags?post=1817"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}