9.) Calculate the coefficient of performance of a carnot refrigerator was 5.0. How much work isrequired to remove and energy of 59.0 kJ from inside the refrigerator.B. 0.0847 kJA. 11.8 kJC. 295 kJD. 64.0 kJE. 54.0 kJ10.) Calculate the change of entropy if 0.5 mole of N2, Hz and He are mixed together. Assume thatthe gases are ideal and they have the same pressure and temperature.A. -1.44 kJB. +1.44 kJC.-12.96 JD. +12.96J

Answered: Image /qna-images/answer/eea5e12e-58ba-4bd5-a1d2-fe06f74cf208.jpg

9.) Calculate the coefficient of performance of a carnot refrigerator was 5.0. How much work is required to remove and energy of 59.0 kJ from inside the refrigerator. A. 11.8 kJ B. 0.0847 kJ C. 295 kJ D. 64.0 kJ E. 54.0 kJ 10.) Calculate the change of entropy if 0.5 mole of N2, Hz and He are mixed together. Assume that the gases are ideal and they have the same pressure and temperature. A. -1.44 kJ B. +1.44 kJ C.-12.96 J D. +12.96 J

9.) Calculate the coefficient of performance of a carnot refrigerator was 5.0. How much work is required to remove and energy of 59.0 kJ from inside the refrigerator. A. 11.8 kJ B. 0.0847 kJ C. 295 kJ D. 64.0 kJ E. 54.0 kJ 10.) Calculate the change of entropy if 0.5 mole of N2, Hz and He are mixed together. Assume that the gases are ideal and they have the same pressure and temperature. A. -1.44 kJ B. +1.44 kJ C.-12.96 J D. +12.96 J

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

Chapter13: Spontaneous Processes And Thermodynamic Equilibrium

Section: Chapter Questions

Problem 46AP

See similar textbooks

Similar questions

Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
For one day, keep a log of all the activities you undertake that consume Gibbs free energy. Distinguish betweenGibbs free energy provided by nutrient metabolism andthat provided by other energy resources.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)