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

10 moles of an ideal gas, in the initial state P1 = 10 atm, T1 = 300K are taken around the following cycle.

a) A reversible change of state along a straight line path on the P-V diagram to the state P = 1 atm T = 300K. How much work is done during the cycle?

2. Relevant equations

Isothermal, ΔU = 0 so w = p dV

3. The attempt at a solution

w = p dV and p = nRT/V so w = nRT (dV/V)

w = nRT ln(Vf/Vi) = nRT ln(Pi/Pf)

w = [(10 moles)* (8.3144 J/ K *mole) * (300K)] ln(10atm/1atm)

w = 57.4 kJ but the correct answer is 123.4kJ. Suggestions??

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# Homework Help: Thermodynamics, Isothermal Question

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