An amount of 2 mole of CO was in the small cubical container of length, (I = a) at 57°C. The gas was taken out completely from the small container and put into large container (1 = 2a) at the same temperature. What is the change in entropy, if it is assumed that the process is reversible and gas is behaving as an ideal gas? A.34.58 J/K B.-34.58 J/K C. -11.53 J/K D. +11.53 J/K The change in entropy accompanying the heating of one mole of helium gas (Cv,n = 3R/2), assumed ideal, from a temperature of 1000 K at constant pressure. (In 2 = 0.7) A. 4.2 cal/K B. 7.0 cal/K C. 2.1 cal/K D. 3.5 cal/K

An amount of 2 mole of CO was in the small cubical container of length, (I = a) at 57°C. The gas was taken out completely from the small container and put into large container (1 = 2a) at the same temperature. What is the change in entropy, if it is assumed that the process is reversible and gas is behaving as an ideal gas? A.34.58 J/K B.-34.58 J/K C. -11.53 J/K D. +11.53 J/K The change in entropy accompanying the heating of one mole of helium gas (Cv,n = 3R/2), assumed ideal, from a temperature of 1000 K at constant pressure. (In 2 = 0.7) A. 4.2 cal/K B. 7.0 cal/K C. 2.1 cal/K D. 3.5 cal/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 1
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