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3. (a) b C. d. e. f. Given 0.01 Molar concentration Au³+ ion and 0.01 molar of Ag+ ion, and the following reaction: T Au³(aq) Ag+ (aq) -→ Au (s) -→ Ag (s) Write the balanced oxidation reduction equation for the cell E° = 1.52 V Eº = 0.80 V Which specie is being oxidized Which Specie is at the anode? Which Specie is the oxidizing agent? Which specie lost electron/s? Which specie saw an increase in oxidation state? Calculate the Ecell at non-standard condition for the reaction

3. (a) b C. d. e. f. Given 0.01 Molar concentration Au³+ ion and 0.01 molar of Ag+ ion, and the following reaction: T Au³(aq) Ag+ (aq) -→ Au (s) -→ Ag (s) Write the balanced oxidation reduction equation for the cell E° = 1.52 V Eº = 0.80 V Which specie is being oxidized Which Specie is at the anode? Which Specie is the oxidizing agent? Which specie lost electron/s? Which specie saw an increase in oxidation state? Calculate the Ecell at non-standard condition for the reaction

Chemistry
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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d, e, f, & g
### Oxidation-Reduction Reaction Analysis Given a 0.01 Molar concentration of Au³⁺ ion and 0.01 molar of Ag⁺ ion, consider the following reactions: - \( \text{Au}^{3+}_{(aq)} \rightarrow \text{Au}_{(s)} \) \( \text{E}^\circ = 1.52 \, \text{V} \) - \( \text{Ag}^+_{(aq)} \rightarrow \text{Ag}_{(s)} \) \( \text{E}^\circ = 0.80 \, \text{V} \) #### Questions (a) Write the balanced oxidation-reduction equation for the cell. (b) Which species is being oxidized? _____________________ (c) Which species is at the anode? _____________________ (d) Which species is the oxidizing agent? _____________________ (e) Which species lost electron(s)? _____________________ (f) Which species saw an increase in oxidation state? _____________________ (g) Calculate the \( \text{E}_{\text{cell}} \) at non-standard conditions for the reaction.
Transcribed Image Text:### Oxidation-Reduction Reaction Analysis Given a 0.01 Molar concentration of Au³⁺ ion and 0.01 molar of Ag⁺ ion, consider the following reactions: - \( \text{Au}^{3+}_{(aq)} \rightarrow \text{Au}_{(s)} \) \( \text{E}^\circ = 1.52 \, \text{V} \) - \( \text{Ag}^+_{(aq)} \rightarrow \text{Ag}_{(s)} \) \( \text{E}^\circ = 0.80 \, \text{V} \) #### Questions (a) Write the balanced oxidation-reduction equation for the cell. (b) Which species is being oxidized? _____________________ (c) Which species is at the anode? _____________________ (d) Which species is the oxidizing agent? _____________________ (e) Which species lost electron(s)? _____________________ (f) Which species saw an increase in oxidation state? _____________________ (g) Calculate the \( \text{E}_{\text{cell}} \) at non-standard conditions for the reaction.
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