∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true? To make this reaction go forward, 33.3 kJ must be added. This reaction is non-spontaneous. This reaction is spontaneous. This reaction cannot be at equilibrium.
∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true? To make this reaction go forward, 33.3 kJ must be added. This reaction is non-spontaneous. This reaction is spontaneous. This reaction cannot be at equilibrium.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy
Section: Chapter Questions
Problem 68SCQ: Explain why each of the following statements is incorrect. (a) Entropy increases in all spontaneous...
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∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true?
To make this reaction go forward, 33.3 kJ must be added. | |
This reaction is non-spontaneous. | |
This reaction is spontaneous. | |
This reaction cannot be at equilibrium. |
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