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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.
(a) 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.
(b) 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

If you don't do your own homework, you won't learn anything, and then who will you get to take your exam for you?!

Answer 2

OK. Let me try to help you. Yes, you need to try hard to do your own homework!
Ideal gas equation should immediately come in to your consideration if the problem is about gas. At STP(0°C and 1.00 atm), 1 mole gas is 22.4L.
(a) At 883°C and 1.00 atm, 1 mole gas is:
0.08206*(273.15+883) = 94.9L
The gas expands from 22.4L to 94.9L at a constant pressure of 1.00 atm, the work done is:
(94.9-22.4)*1.00 = 72.5atm·L = 7.35 kJ

(b) That means the energy initially used to do the work of expansion would be used instead to heat up the gas further. Please pay attention to the unit difference, since 7.35 kJ is for one mol N2 = 28g, but the specific heat capacity of N2 is 1.00 J/g·K:
(7.35 kJ/Mol)/(28g/Mol)/(1.00 J/g·K) = 262K
262K is the temperature change if the gas were heated with the same amount of energy in a container of fixed volume.