{"id":3526,"date":"2019-09-25T07:00:52","date_gmt":"2019-09-25T07:00:52","guid":{"rendered":"http:\/\/flowactivo.org\/?p=3526"},"modified":"2019-09-25T07:00:52","modified_gmt":"2019-09-25T07:00:52","slug":"what-are-the-gas-laws-in-chemistry","status":"publish","type":"post","link":"https:\/\/flowactivo.org\/de\/what-are-the-gas-laws-in-chemistry\/","title":{"rendered":"What are the Gas Laws in Chemistry?"},"content":{"rendered":"

The gas laws can be used to predict the behaviour of gases under certain physical conditions. Examples of gas laws include Charles\u2019 law, Boyle\u2019s law<\/a>, and Gay-Lussac\u2019s law. These laws provide relationships between:
\nThe pressure exerted by gaseous substances on the walls of their containers (often denoted by \u2018P\u2019)
\nThe absolute temperature associated with the gas (denoted by the symbol \u2018T\u2019 and expressed in Kelvin)
\nThe number of moles of gas or the amount of gaseous substance (generally denoted by \u2018n\u2019)
\nThe volume occupied by the gas (often denoted by the symbol \u2018V\u2019 and expressed in terms of litres)
\nA brief description of three of the gas laws is provided in this article.
\nBoyle\u2019s Law<\/strong>
\nBoyle\u2019s law states that the pressure exerted by a gas on its container increases as the volume of the container decreases (when the absolute temperature of the gas and the number of gaseous moles are constant).
\nThe mathematical expression of this law is:
\nP = k\/V (or) PV = k
\nWhere P is the pressure associated with the gas, V is the volume of the gas, and k is a constant.
\nCharles\u2019 Law<\/strong>
\nCharles\u2019 law can be stated as follows – \u201cWhen the number of gaseous moles and the pressure of the gas is kept constant, the volume occupied by a gaseous substance is directly proportional to the absolute temperature associated with the gas\u201d.
\nThis law can be expressed as follows:
\nV\/T = k (or) V = kT
\nWhere V is the volume occupied by the gas, T is the absolute temperature of the gas, and k is a constant.
\nAvogadro\u2019s Law<\/strong>
\nA relationship between the number of moles of a gas and the volume occupied by the gas is provided by Avogadros law<\/a>. This law can be stated as follows – \u201cwhen the absolute temperature of a gas and the pressure associated with it are kept constant, the number of moles of a gaseous substance is directly proportional to the volume occupied by it\u201d.
\nThis law can be expressed via the following equation:
\nV\/n = k (or) V = k*n
\nWhere V is the volume of the gas, n is the number of moles of gas, and k is a constant. To learn more about the gas laws and other interesting concepts in chemistry, subscribe to the BYJU\u2019S YouTube channel and enable notifications.
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