Asked by Jake
. At 1.00 atm, one mole of nitrogen gas is heated from 0 to 819°C in a cylinder constrained by a weightless piston. (a) Determine the joule value of the gas's work of expansion. Assume that all the energy is spent on work. (b) What would happen if the gas was heated with the same amount of energy in a container with a fixed volume? (Average specific heat capacity of N2 is 1.04 J/g*K.)
Answers
Answered by
DrBob222
a.
Volume 1 mole N2 @ zero C =22.4 L
Volume 1 mole N2 @ 819 C (or 1092 K) = V =nRT/P = 1*0.08206*1092/1 = 80.6 L
delta V = 80.6 - 22.4 = 58.2 L
Then work = -pdV = -1*58.2 = -58.2 L*atm
-58.2 L*atm x 101.325 = ? J.
b.
If the volume is fixed then delta V = 0 and -pdV = 0
Volume 1 mole N2 @ zero C =22.4 L
Volume 1 mole N2 @ 819 C (or 1092 K) = V =nRT/P = 1*0.08206*1092/1 = 80.6 L
delta V = 80.6 - 22.4 = 58.2 L
Then work = -pdV = -1*58.2 = -58.2 L*atm
-58.2 L*atm x 101.325 = ? J.
b.
If the volume is fixed then delta V = 0 and -pdV = 0
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.