# Thermodynamics: Compression of an Adiabatic Gas

Minescrushessouls

## Homework Statement

Assume 1.500 mol of a monatomic ideal gas is compressed from 3.00 L to 1.00 L.

a. If the initial and final temperature is 10.0 °C, what are the initial and final pressures (in atm)?

b. How much work input (in kJ) is required if a reversible isothermal path at 10.0 °C is followed?

c. How much work input (in kJ) is required if the compression is adiabatic rather than isothermal? Assume the initial temperature is 10.0 °C.

PV=nRT
w=-nRTln(vf/vi)
U=q+w

## The Attempt at a Solution

I got both a and b using the first two equations I listed. I got the inital pressure to be 11.6 atm and the final pressure to be 34.8 atm. For the second part I got the work to be 3.88 kJ.

I'm stuck on the third part. I know adiabatic means that there no change in U, so q=-w but I don't know how that applies to the question.