Isobaric Process: Finding Work Done by Ideal Gas

[tigers4]

Homework Statement

When 23.3 J was added as heat to a particular ideal gas, the volume of the gas changed from 54.7 cm³ to 100 cm³ while the pressure remained at 1.00 atm.
(a) By how much did the internal energy of the gas increase?
J

(b) If the quantity of gas present was 2.00 10-3 mol, find Cp.
J/mol·K

(c) Find CV.
J/mol·K

Homework Equations

PV=nRT
C_p=C_v+R
E_int=C_vRT

The Attempt at a Solution

I have tried to use the equations above but am not sure how to calculate the temperature in kelvin from Joules

 

[kuruman]

What kind of process is this, constant volume, constant pressure, isothermal or adiabatic?

 

[tigers4]

constant pressure

 

[kuruman]

Correct. What does the first law of thermodynamics say?

 

[tigers4]

change in internal energy U=Q-W
change in internal energy=heat added-work done by system

 

[kuruman]

change in internal energy U=Q-W
change in internal energy=heat added-work done by system

Correct. You know that 23.3 J of heat was added to the gas. If you can find W, the work done by the system, then you have the change in internal energy. How does one find the work done by the system (gas) when one has a constant pressure process?