A disproportionation reaction involves a substance that acts as both an oxidizing and reducing agent, producing higher and lower oxidation states of the same element in the products. Which of the following disproportionation reactions are spontaneous under standard conditions? Calculate ΔG° and K at 25°C for those reactions that are spontaneous under standard conditions. Use the following half-reactions. (Enter ΔG° = 0 and K= 0 for reactions that are not spontaneous.) ClO3- + 3 H+ + 2e- → HClO2 + H2O ℰ° = 1.21 VHClO2 + 2 H+ + 2e- → HClO + H2O ℰ° = 1.65 V (a) 2 Cu+(aq) → Cu2+(aq) + Cu(s) spontaneous or not spontaneous ? ΔG° -34.7 kJ K ? I found that G is correct and because it is negative it is spontaneous. Could you please help me figure out K?
A disproportionation reaction involves a substance that acts as both an oxidizing and reducing agent, producing higher and lower oxidation states of the same element in the products. Which of the following disproportionation reactions are spontaneous under standard conditions? Calculate ΔG° and K at 25°C for those reactions that are spontaneous under standard conditions. Use the following half-reactions. (Enter ΔG° = 0 and K= 0 for reactions that are not spontaneous.) ClO3- + 3 H+ + 2e- → HClO2 + H2O ℰ° = 1.21 VHClO2 + 2 H+ + 2e- → HClO + H2O ℰ° = 1.65 V (a) 2 Cu+(aq) → Cu2+(aq) + Cu(s) spontaneous or not spontaneous ? ΔG° -34.7 kJ K ? I found that G is correct and because it is negative it is spontaneous. Could you please help me figure out 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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A disproportionation reaction involves a substance that acts as both an oxidizing and reducing agent, producing higher and lower oxidation states of the same element in the products. Which of the following disproportionation reactions are spontaneous under standard conditions? Calculate ΔG° and K at 25°C for those reactions that are spontaneous under standard conditions. Use the following half-reactions. (Enter ΔG° = 0 and K= 0 for reactions that are not spontaneous.)
ClO3- + 3 H+ + 2e- → HClO2 + H2O ℰ° = 1.21 V
HClO2 + 2 H+ + 2e- → HClO + H2O ℰ° = 1.65 V
HClO2 + 2 H+ + 2e- → HClO + H2O ℰ° = 1.65 V
(a) 2 Cu+(aq) → Cu2+(aq) + Cu(s)
spontaneous or not spontaneous ?
| ΔG° | -34.7 kJ |
| K | ? |
I found that G is correct and because it is negative it is spontaneous. Could you please help me figure out K?
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