One mole of nitrogen (N2) is cooled from an initial temperature and pressure of 700 K and 10 bar to a final temperature of 300 K. The heat capacity of nitrogen may be taken as: Cp,m = 28.58 + 3.77 × 10-3 T where Cp,m is in J mol-1 K-1 and T is in Kelvin. Assuming nitrogen behaves as an ideal gas, calculate q, w, ∆U, and ∆H for this process when it is carried out (a) at constant pressure, and (b) at constant volume. Compare the values obtained for the two cases.

One mole of nitrogen (N2) is cooled from an initial temperature and pressure of 700 K and 10 bar to a final temperature of 300 K. The heat capacity of nitrogen may be taken as: Cp,m = 28.58 + 3.77 × 10-3 T where Cp,m is in J mol-1 K-1 and T is in Kelvin. Assuming nitrogen behaves as an ideal gas, calculate q, w, ∆U, and ∆H for this process when it is carried out (a) at constant pressure, and (b) at constant volume. Compare the values obtained for the two cases.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 21P

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