Help i'm stuck on a thermodynamics(heat engine) problem
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A piston contains 100 moles of an ideal monatomic gas that initally has a pressure of 2.19 × 105 Pa and a volume of 2.7 m3. The piston is connected to a hot and cold reservoir and the gas goes through the following quasi-static cycle accepting energy from the hot reservoir and exhausting energy into the cold reservoir.
The pressure of the gas is increased to 5.19 × 105 Pa while maintaining a constant volume.
The volume of the gas is increased to 9.7 m3 while maintaining a constant pressure.
The pressure of the gas is decreased to 2.19 × 105 Pa while maintaining a constant volume.
The volume of the gas is decreased to 2.7 m3 while maintaining a constant pressure.
It may help you to recall that CV = 12.47 J/K/mole and CP = 20.79 J/K/mole for a monatomic ideal gas, and that the number of gas molecules is equal to Avagadros number (6.022 × 1023) times the number of moles of the gas.
The question asks, How much energy is transferred into the gas from the hot reservoir?
So i know we have to use PV=nRT to solve for initial temp
T = PV/nR
i have done this and the T initial comes out as 711.14 K
Now i have to calculate for delta T when the pressure increases (step 1, constant V)
and also delta T when the volume increases (step 2, constant P)