for an isobaric process the ratio of delta q to the delta w is
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In a reversible isobaric process, you are adding heat to the gas Q and it is expanding at constant pressure P to do reversible work on its surroundings. So:
W=PΔV
ΔU=Q−W=Q−PΔV
But, from the ideal gas law, PV=nRT, so
W=nRΔT(1)
and
ΔU=Q−nRΔT
So,
Q=ΔU+nRΔT
But for an ideal gas:
ΔU=nCvΔT(2)
So,
Q=nCvΔT+nRΔT=nR(Cv+R)ΔT=nCpΔT(3)
Therefore, from Eons. 1-3, we have:
Q:ΔU:W=nCpΔT:nCvΔT:nRΔT
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