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 & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section: Chapter Questions
Problem 100GQ: Copper(I) ion disproportionates to copper metal and copper(ll) ion. (See Study Question 99.) 2...
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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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