(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

two moles of an ideal gas is initially at P = 2*20^5 Pa expands adiabaticaly to four times its original volume. it is then compressed at constant pressure to its original volume. what is the change in entropy of the gas

Cp = 20.78 joules/mole-deg

Cv = 12.47 joules/mole-deg

gamma = 5/3

2. Relevant equations

adiabatic expansion --> PV^gamma = constant, Q = 0

isovolumetric compression --> nCv(deltaT)

entropy deltaS= deltaQ/T

3. The attempt at a solution

i am not sure how to use the adiabatic equation because although P and V is given aswell as gamma, i can solve for 'constant' but where does constant come into play?

since for an adiabat Q = 0, do i just take it as zero and move on or do i actually need to solve for something.

as for the isovolumetric compression, moles is given, Cv is given but not deltaT so i solved the Pv=nRT eq for T and subbed it in, i then assumed P and V to be constants as stated in the problem?? and solved for Q getting 1.5 joules

when i solved for entropy i did (compression - expansion, so isovolumetric minus adibat = i subbed in the equation from the isovolumetric equation in and cancelled out the T's and was able to get deltaS = 24.94 joules per kelvin

did i take the correct approach? help appreciated...

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# Homework Help: Ideal gas adiabatic/isovolumetric help

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