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Charles’ Law

Charles’ Law describes the relationship between the change in volume and the temperature of a gas. For an ideal gas, the volume and temperature of a gas are directly proportional if the pressure and number of moles are constant. Thus, this explains why the volume increases as the temperature of the gas increases, regardless of their differing chemical properties.

Charles’ Gas Law is commonly written as:

V = k*T

V is the volume of the gas
k is a constant
T is the temperature of gas

For example, if the temperature of molecular oxygen halves, with pressure and number of moles remaining constant, the volume of this particular gas should also halve. This phenomenon should apply to all gases, as volume is directly proportional to temperature. So doubling the temperature of molecular hydrogen should also double its volume.

Charles’ Gas Law has been used in conjunction with Boyle’s Law and Gay-Lussac’s Law to form the Combined Gas Law, which has itself been combined with Avogadro’s Law to form the Ideal Gas Law. The Ideal Gas Law still considers the relationship between volume and temperature, but it also includes the new variables pressure and number of moles. Thus, understanding Charles’ Law is crucial to understanding how the volume and temperature are related; and by extension its function in the Ideal Gas Law.


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Charles' Law, Gay-Lussac's Law & Combined Gas Law

1. What is the final volume of argon gas if 2.50 L at 705 torr is compressed to a pressure of 1550 torr? Assume the temperature remains constant. 2. Calculate the volume of chlorine gas at 20°C and 75.0 cm Hg if the volume of the gas is 1.10 L at 20°C and 95.5 cm Hg. Charles' Law: 3. What is the final Celsius temperature if

Charles Law Concept Questions.

I included Charles law lab procedures for reference and questions are in MS words format. (See attached files for full problem description) --- 1. When the flask is submerged in the boiling water, what is happening to the gas inside the flask? 2. Compare the pressure of the gas outside the flask with the pressure of the