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Starting with 2.50mol of N2 gas (assumed to be ideal) in a cylinder at 1.00 atm...

Starting with 2.50mol of N2 gas (assumed to be ideal) in a cylinder at 1.00 atm and 20.0 C, a chemist first heats the gas at constant volume, adding 1.36 X 10^4 J of heat, then continues heating and allows the gas to expand at constant pressure to twice its original volume.

(A) Calculate the final temperature of the gas. (Book Answer says: 837 C)

(B) Calculate the amount of work done by the gas. (Book Answer says: 11.5 kJ)

(C) The amount of heat added to the gas while it was expanding. (Book Answer says: 40.3 kJ)

(D) The change in internal energy of the gas for the whole process. (Book Answer says: 42.4 kJ)

I cannot get these answers, thank you for the help.

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