An ideal gas expands at a constant total pressure of 2.5 atm from 500mL to 750mL

Question

An ideal gas expands at a constant total pressure of 2.5 atm from 500mL to 750mL. Heat then flows out of the gas at constant volume, and the pressure and temp are allowed to drop until the temp reaches its original value.
Part A: calculate the total work done by the gas in the process?
Part B: calculate the total heat flow into the gas. An ideal gas expands at a constant total pressure of 2.5 atm from 500mL to 750mL. Heat then flows out of the gas at constant volume, and the pressure and temp are allowed to drop until the temp reaches its original value.
Part A: calculate the total work done by the gas in the process?
Part B: calculate the total heat flow into the gas.
Part A: calculate the total work done by the gas in the process?
Part B: calculate the total heat flow into the gas.

Explanation / Answer

2.5 atm from 500mL to 750mL

A. work=P*delta V=2.5*(0.75-0.5)=2.5*0.25=0.625 atm L

1 atm L =0.101325 kilojoules

0.625 atm L =0.063328125 kilojoules=63.32 J

B U = n?Cv?T
Since the gas return to its initial temperature, the total change of internal energy on this whole process is zero:
?U = n?Cv??T = 0

On the other hand the change of internal energy equal the sum of heat transferred to the gas plus the work done on it.
?U = Q + W = 0

Hence;
Q = - W = - (-63.32j) = 63.32J

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