Two identical cylinders each contain the same amount of the same ideal gas with the same initial temperature, Tlow. The gas in the first cylinder undergoes an isovolumetric pressure increase and reaches a final temperature of Thigh. The gas in the second cylinder undergoes an isobaric expansion reaching the same final temperature, Thigh. What is the ratio of the change of entropy of the gas in the first cylinder to the change of entropy of the gas in the second cylinder? (∆S1/∆S2 = ?)
1st cylinder :
change at constant volume
we know that
at constant volume
dS = nCv ln (T2 / T1)
so
in this case
dS1 = nCv ln (Thigh / T1)
2nd cylinder :
change at constant pressure
we know that
at constant pressure
dS = nCp ln (Thigh / T1)
so
in this case
dS2 = nCp ln ( Thigh / T1)
now
dS1 / dS2 = nCv ln (Thigh / T1) / nCp ln ( Thigh /
T1)
so
dS1 / dS2 = Cv / Cp
so
the ratio os Cv / Cp of the gas
where
Cv = molar specific heat at constant volume
Cp = molar specific heat at constant pressure
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