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## Homework Statement

[/B]50 moles of an ideal gas for which Cp= 5/2R and Cv=3/2R initially has a pressure of 1x10^5 Pa, and a volume of 1.0m^3. It undergoes a process where the pressure and volume both double while they stay proporitional to each other: P=constV. What is the change in temperature for this process?

## Homework Equations

ΔU= Q-W

PV=nRΔT

ΔU= nCv(ΔT) [/B]

## The Attempt at a Solution

So I started by trying to use PV=nRΔT and calculating T, however I wasnt successful. The answer in my book is in Kelvins, so I tried converting the temperature that I calculated to Kelvins, however it was still wrong.

I'm thinking that I might need to take the integral: ∫ PVdv but im not sure if thats correct either.

Can somone please help me out, It would be greatly appreciated.

**The correct answer is: 720K**

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