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.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
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