Given AH°= +500 kJ/mol and the equilibrium constant, K = 1 x 10-10 , which of the following is correct concerning the following system at equilibrium at 298 Kelvin? A + B=C + D A) AG = 0 B) AG° = 0 C) AG° < 0 D) The reaction is exothermic. E) This is a product-favored reaction.

Given AH°= +500 kJ/mol and the equilibrium constant, K = 1 x 10-10 , which of the following is correct concerning the following system at equilibrium at 298 Kelvin? A + B=C + D A) AG = 0 B) AG° = 0 C) AG° < 0 D) The reaction is exothermic. E) This is a product-favored reaction.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.95QE: Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at...

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