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1. Consider a galvanic cell constructed from the following half-cells at 298 K. Half-cell 1: Graphite electrode in a solution that is 0.0010 M Mn04¬, 0.20 M Mn²+, with pH = 2.00 Mn04 (aq) + 8H*(aq) + 5e- → Mn²*(aq) + 4H20(1) E° = 1.51 V Half-cell 2: Copper electrode in 0.50 M Cu²+ Cu2*(aq) + 2e- → Cu(s) E° = 0.34 V Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow. а. KNO3 salt bridge ANODE HALF-CELL CATHODE HALF-CELL b. Write the line notation for the cell.

1. Consider a galvanic cell constructed from the following half-cells at 298 K. Half-cell 1: Graphite electrode in a solution that is 0.0010 M Mn04¬, 0.20 M Mn²+, with pH = 2.00 Mn04 (aq) + 8H*(aq) + 5e- → Mn²*(aq) + 4H20(1) E° = 1.51 V Half-cell 2: Copper electrode in 0.50 M Cu²+ Cu2*(aq) + 2e- → Cu(s) E° = 0.34 V Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow. а. KNO3 salt bridge ANODE HALF-CELL CATHODE HALF-CELL b. Write the line notation for the cell.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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1. Consider a galvanic cell constructed from the following half-cells at 298 K. Half-cell 1: Graphite electrode in a solution that is 0.0010 M Mn04, 0.20 M Mn2+, with pH = 2.00 %3D Mn04 (aq) + 8H*(aq) + 5e → Mn²+(aq) + 4H20(1) E° = 1.51 V Half-cell 2: Copper electrode in 0.50 M Cu²+ Cu2*(aq) + 2e- → Cu(s) E° = 0.34 V %3D a. Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow. KNO3 salt bridge ANODE HALF-CELL САТHODE HALF-CELL b. Write the line notation for the cell. c. Write the balanced cell reaction and the equilibrium constant (K) for the cell reaction. d. Calculate the cell potential (E) and AG.
Transcribed Image Text:1. Consider a galvanic cell constructed from the following half-cells at 298 K. Half-cell 1: Graphite electrode in a solution that is 0.0010 M Mn04, 0.20 M Mn2+, with pH = 2.00 %3D Mn04 (aq) + 8H*(aq) + 5e → Mn²+(aq) + 4H20(1) E° = 1.51 V Half-cell 2: Copper electrode in 0.50 M Cu²+ Cu2*(aq) + 2e- → Cu(s) E° = 0.34 V %3D a. Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow. KNO3 salt bridge ANODE HALF-CELL САТHODE HALF-CELL b. Write the line notation for the cell. c. Write the balanced cell reaction and the equilibrium constant (K) for the cell reaction. d. Calculate the cell potential (E) and AG.
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