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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![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3803c08e-019f-4a2b-95b8-8d25790d454e%2Fc3e35947-36ef-4d12-8efd-ce41c188ed36%2Fgbox99e_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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
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