Chem help?

Question

One mole of nitrogen gas confined within a cylinder by a piston is heated from 0°C to 883°C at 1.00 atm.

Calculate the work of expansion of the gas in joules (1 J = 9.87 10-3 atm·L). Assume all the energy is used to do work.

What would be the temperature change if the gas were heated with the same amount of energy in a container of fixed volume? (Assume the specific heat capacity of N2 is 1.00 J/g·K.)

Answer 1

Wow, you are even given a conversion factor!
So, one mole of nitrogen gas was originally at STP (0°C & 1.00 atm), its volume was 22.4L.
When it is heated to 883°C, the new volume is:
V = RT/P = 0.08206*(883+273)/1 = 94.9L
Thus the work of expansion of the gas is:
1*(94.9 - 22.4)/9.87x10-3 = 7.345 (kJ)

If this amount of energy is used to heat up the gas (without doing work):
(7.345 kJ)/(1.00 J/g·K*28g) = 262K
Thus the temperature would be 262K higher, to 1145C