Consider the following reaction AgBr(s) → Ag+(aq) + Br−(aq), ΔGo = +69.1 kJ Calculate ΔG for the reaction when [Ag+] = 1.0 × 10−2 M and [Br−] = 1.0 × 10−3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? ΔG = 40.6 kJ, nonspontaneous ΔG = 69.1 kJ, nonspontaneous ΔG = −97.5 kJ, spontaneous ΔG = −40.6 kJ, nonspontaneous ΔG = −69.1 kJ, spontaneous ΔG = 97.5 kJ, spontaneous
Consider the following reaction AgBr(s) → Ag+(aq) + Br−(aq), ΔGo = +69.1 kJ Calculate ΔG for the reaction when [Ag+] = 1.0 × 10−2 M and [Br−] = 1.0 × 10−3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? ΔG = 40.6 kJ, nonspontaneous ΔG = 69.1 kJ, nonspontaneous ΔG = −97.5 kJ, spontaneous ΔG = −40.6 kJ, nonspontaneous ΔG = −69.1 kJ, spontaneous ΔG = 97.5 kJ, spontaneous
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the following reaction
AgBr(s) → Ag+(aq) + Br−(aq), ΔGo = +69.1 kJ
Calculate ΔG for the reaction when [Ag+] = 1.0 × 10−2 M and [Br−] = 1.0 × 10−3 M. Is the reaction spontaneous or nonspontaneous at these concentrations?
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ΔG = 40.6 kJ, nonspontaneous |
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ΔG = 69.1 kJ, nonspontaneous |
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ΔG = −97.5 kJ, spontaneous |
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ΔG = −40.6 kJ, nonspontaneous |
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ΔG = −69.1 kJ, spontaneous |
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ΔG = 97.5 kJ, spontaneous |
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