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Consider the electrochemical cell: Cu/10-4 M Cu²+, 1M H*/Pt/H₂ (a=1). Determine the equilibrium potential versus the indicated reference electrode. a. 0.342 V. b. 0.082 V. c. 0.222 V. 0.462 V.

Consider the electrochemical cell: Cu/10-4 M Cu²+, 1M H*/Pt/H₂ (a=1). Determine the equilibrium potential versus the indicated reference electrode. a. 0.342 V. b. 0.082 V. c. 0.222 V. 0.462 V.

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
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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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### Electrochemical Cell and Reaction Calculations #### Problem 5 Consider the electrochemical cell: Cu/10^-4 M Cu^2+, 1M H^+/Pt/H2 (a=1). Determine the equilibrium potential versus the indicated reference electrode. - a. 0.342 V - b. 0.082 V - c. 0.222 V - d. 0.462 V #### Problem 6 Consider the reaction, Fe^3+ + e^- = Fe^2+. The exchange current density, i₀, for the reaction on Pt is 0.005 mA/cm² and the transfer coefficient is 0.50. Calculate the current density of the reaction at 0.971 V. - a. 2450 mA/cm² - b. 245 mA/cm² - c. 24.5 mA/cm² - d. 2.45 mA/cm² This content challenges students to apply principles of electrochemistry, specifically in determining equilibrium potentials and calculating current densities based on given parameters.
Transcribed Image Text:### Electrochemical Cell and Reaction Calculations #### Problem 5 Consider the electrochemical cell: Cu/10^-4 M Cu^2+, 1M H^+/Pt/H2 (a=1). Determine the equilibrium potential versus the indicated reference electrode. - a. 0.342 V - b. 0.082 V - c. 0.222 V - d. 0.462 V #### Problem 6 Consider the reaction, Fe^3+ + e^- = Fe^2+. The exchange current density, i₀, for the reaction on Pt is 0.005 mA/cm² and the transfer coefficient is 0.50. Calculate the current density of the reaction at 0.971 V. - a. 2450 mA/cm² - b. 245 mA/cm² - c. 24.5 mA/cm² - d. 2.45 mA/cm² This content challenges students to apply principles of electrochemistry, specifically in determining equilibrium potentials and calculating current densities based on given parameters.
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