One mole of N2 at 293.5 K and 5.29 bar undergoes a transformation to a state described by 418 K and 4.53 bar. Calculate the entropy change for the process (J/K) if Cp is as follows: C, P,m = 30.81 – 11.87 × 10-3T+2.3968 × 10-$T2 – 1.0176× 10-87³ J/mol – K

One mole of N2 at 293.5 K and 5.29 bar undergoes a transformation to a state described by 418 K and 4.53 bar. Calculate the entropy change for the process (J/K) if Cp is as follows: C, P,m = 30.81 – 11.87 × 10-3T+2.3968 × 10-$T2 – 1.0176× 10-87³ J/mol – K

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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Question

One mole of N2 at 293.5 K and 5.29 bar undergoes a transformation to a state described by 418 K and 4.53 bar.
Calculate the entropy change for the process (J/K) if Cp is as follows:
C, =30.81 – 11.87 × 10-3T+2.3968 × 10-$T2 – 1.0176× 10-8T³ J/mol – K
P,m
Ans. in 3SFS

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