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What is Gay-Lussac's Law?

Gay-Lussac's Law is the third and final of the laws leading up to the ideal gas law. The first is Boyle's Law, which gives the relationship between volume and pressure, and the second is Charles' Law, which gives the relationship between volume and temperature. Gay-Lussac's Law has also been referred to as Charles' Law, but they are not the same.

The founder of this particular thermodynamic relation is Joseph Gay-Lussac (1785-1850). He not only rescued Charles' Law from oblivion by duplicating the experiments and publishing the results, but re-created similar conditions to find the connection between pressure and temperature. Gay-Lussac found that for a gas, if the pressure increases, the temperature increases, and if the temperature increases, so does the pressure.

The Equation

According to Gay-Lussac's Law, at constant volume V, the pressure P is directly proportional to the temperature T:

1) P ˜ T

or

2) P = kT where k = constant

Rewriting equation 2, we have:

3) P/T = constant

Gay-Lussac's Law is also commonly written as:

4) P1/T1 = P2/T2

where P1 and T1 are the original values of the gas, while P2 and T2 represent its final values. In addition to the pressure being constant, the same caveats used in any ideal gas law apply here. These results apply for systems where an equilibrium state has been reached, the gas is not too dense, and P is around atmospheric pressure. Real gases approximate these conditions enough such that the law is applicable in every day life.

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http://www.brighthub.com/engineering/mechanical/articles/26213.aspx#ixzz0T9mVS0Iz**Charles' Law ** is named after Jacques Charles (1746-1823), who discovered it but did not publish his findings. Mankind is able to benefit from his work due to the efforts of Joseph Gay-Lussac, who also used this result to fuel his own eponymous discovery.

The Equation

According to Charles' Law, at constant pressure P, the volume V is directly proportional to the temperature T:

1) V ˜ T

or

2) V = kT, where k is a constant

Rewriting equation 2, we have:

3) V/T = constant

Charles' Law is also commonly written as:

4) V1/T1 = V2/T2

where V1 and T1 are the original values of the gas, while V2 and T2 represent its final values.

In addition to the pressure being constant, the same caveats used in any ideal gas law apply here. These results apply for systems where an equilibruim state has been reached, the gas is not too dense, and P is around atmospheric pressure. Real gases approximate these conditions enough such that the law is applicable in every day life.