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

Initially, 0.745 moles of an ideal gas in a container occupies a volume of 3.55 L at a pressure of 3.82 atm with an internal energy of 1705 J. The gas is then cooled at a constant volume until its pressure is 2.06 atm. Then the gas is allowed to expand at a constant pressure until its volume is 6.65 L. The final internal energy is 2098 J. Consider the processes to be quasi-static. What is the work associated with this entire process?

2. Relevant equations

W=-P*deltaV

deltaU=Q + W

3. The attempt at a solution

Is it correct that you take the 2.06, multiply it by 1E5, and multiply the answer by the change in volume in m^3 to find -638.60 J

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# Homework Help: Thermodynamic Problems: Work and Heat in a Thermodynamic Process

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