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) + 4H2O(1) E° = 1.51 V Half-cell 2: Copper electrode in 0.50 M Cu²+ Cu2*(aq) + 2e¯ → Cu(s) E° = 0.34 V a. Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow. KNO3 salt bridge ANODE HALF-CELL CATHODE 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.
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) + 4H2O(1) E° = 1.51 V Half-cell 2: Copper electrode in 0.50 M Cu²+ Cu2*(aq) + 2e¯ → Cu(s) E° = 0.34 V a. Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow. KNO3 salt bridge ANODE HALF-CELL CATHODE 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.
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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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 MnO4¯, 0.20 M Mn2+, with pH = 2.00
Mn04 (aq) + 8H*(aq) + 5e¯ → Mn²*(aq) + 4H2O(1)
E° = 1.51 V
Half-cell 2:
Copper electrode in 0.50 M Cu²+
Cu2*(aq) + 2e- → Cu(s)
E° = 0.34 V
a. Fill in the diagram. Label the electrode charges, current flow, anion flow, and cation flow.
KNO3 salt bridge
ANODE HALF-CELL
CATHODE 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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