The standard cell potential, E298° = -1.334 V, for the half-cell reaction Pb (s) + 2 H₂O (/) = PbO₂ (s) + 4 H+ (aq) + 4e¯ . (a) Using additional tabulated data as needed, calculate £298° (in V) for the half-cell, Pb²+ (aq) + 2 H₂O (1) PbO₂ (s) + 4 H+ (aq) + 2 e¯. (b) Use the cell potentials given or determined in this problem to find Kc for the reaction, 2 Pb²+ (aq) + 2 H₂O (/) = Pb (s) + PbO₂ (s) + 4 H+ (aq) .
The standard cell potential, E298° = -1.334 V, for the half-cell reaction Pb (s) + 2 H₂O (/) = PbO₂ (s) + 4 H+ (aq) + 4e¯ . (a) Using additional tabulated data as needed, calculate £298° (in V) for the half-cell, Pb²+ (aq) + 2 H₂O (1) PbO₂ (s) + 4 H+ (aq) + 2 e¯. (b) Use the cell potentials given or determined in this problem to find Kc for the reaction, 2 Pb²+ (aq) + 2 H₂O (/) = Pb (s) + PbO₂ (s) + 4 H+ (aq) .
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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https://chem.libretexts.org/Ancillary_Materials/Reference/Reference_Tables/Electrochemistry_Tables/P1%3A_Standard_Reduction_Potentials_by_Element
![### Understanding Standard Cell Potential and Calculations
**The Standard Cell Potential:**
The standard cell potential, \( \varepsilon_{298}^\circ = -1.334 \, \text{V} \), is provided for the following half-cell reaction:
\[ \text{Pb (s)} + 2 \, \text{H}_2\text{O (l)} \rightleftharpoons \text{PbO}_2 \, \text{(s)} + 4 \, \text{H}^+ \, \text{(aq)} + 4 \, \text{e}^- \, . \]
**Task (a): Calculation Using Tabulated Data**
Using additional tabulated data as needed, calculate \( \varepsilon_{298}^\circ \) (in V) for the half-cell reaction:
\[ \text{Pb}^{2+} \, \text{(aq)} + 2 \, \text{H}_2\text{O (l)} \rightleftharpoons \text{PbO}_2 \, \text{(s)} + 4 \, \text{H}^+ \, \text{(aq)} + 2 \, \text{e}^- \, . \]
**Task (b): Determining the Equilibrium Constant**
Use the cell potentials given or determined in this problem to find the equilibrium constant \( K_c \) for the reaction:
\[ 2 \, \text{Pb}^{2+} \, \text{(aq)} + 2 \, \text{H}_2\text{O (l)} \rightleftharpoons \text{Pb (s)} + \text{PbO}_2 \, \text{(s)} + 4 \, \text{H}^+ \, \text{(aq)} \, . \]
**Explanation of Graphs or Diagrams:**
There are no graphs or diagrams in the provided image, only chemical equations and numerical data related to standard cell potential calculations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3c924432-5356-4d2a-9799-f03f3a53c4ab%2F75c12299-8b14-4ac0-a90a-bbc522a38116%2Fcx8vw3i_processed.png&w=3840&q=75)
Transcribed Image Text:### Understanding Standard Cell Potential and Calculations
**The Standard Cell Potential:**
The standard cell potential, \( \varepsilon_{298}^\circ = -1.334 \, \text{V} \), is provided for the following half-cell reaction:
\[ \text{Pb (s)} + 2 \, \text{H}_2\text{O (l)} \rightleftharpoons \text{PbO}_2 \, \text{(s)} + 4 \, \text{H}^+ \, \text{(aq)} + 4 \, \text{e}^- \, . \]
**Task (a): Calculation Using Tabulated Data**
Using additional tabulated data as needed, calculate \( \varepsilon_{298}^\circ \) (in V) for the half-cell reaction:
\[ \text{Pb}^{2+} \, \text{(aq)} + 2 \, \text{H}_2\text{O (l)} \rightleftharpoons \text{PbO}_2 \, \text{(s)} + 4 \, \text{H}^+ \, \text{(aq)} + 2 \, \text{e}^- \, . \]
**Task (b): Determining the Equilibrium Constant**
Use the cell potentials given or determined in this problem to find the equilibrium constant \( K_c \) for the reaction:
\[ 2 \, \text{Pb}^{2+} \, \text{(aq)} + 2 \, \text{H}_2\text{O (l)} \rightleftharpoons \text{Pb (s)} + \text{PbO}_2 \, \text{(s)} + 4 \, \text{H}^+ \, \text{(aq)} \, . \]
**Explanation of Graphs or Diagrams:**
There are no graphs or diagrams in the provided image, only chemical equations and numerical data related to standard cell potential calculations.
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