The potential of the following voltaic cell is 0.55 V. Given this information, determine the Kb for the organic base (RNH2) dissolved in the left cell.
The potential of the following voltaic cell is 0.55 V. Given this information, determine the Kb for the organic base (RNH2) dissolved in the left cell.
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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The potential of the following voltaic cell is 0.55 V. Given this information, determine
the Kb for the organic base (RNH2) dissolved in the left cell.
![The given image depicts a galvanic cell notation and a table containing standard electrode potentials.
**Galvanic Cell Notation:**
- The cell notation is written as:
\( \text{Pt (s) } \| \text{ H}_2 \text{ (g) (0.85 atm) } \| \text{ RNH}_2 \text{ (aq) (0.10 M), RNH}_3\text{Cl (aq) (0.050 M) } \| \text{ SHE} \).
This notation describes a galvanic cell consisting of:
- A platinum electrode (Pt \((s)\))
- Hydrogen gas (\( \text{H}_2 \)), at a pressure of 0.85 atm
- An aqueous solution containing RNH\(_2\) at 0.10 M and RNH\(_3\)Cl at 0.050 M
- The Standard Hydrogen Electrode (SHE) as the reference
**Table of Half-Reactions:**
- The table presents the electrochemical half-reactions along with their standard electrode potentials \(E^\circ\).
1. The first half-reaction:
\[
2 \text{H}^+ \text{ (aq)} + 2 \text{e}^- \rightleftharpoons \text{H}_2 \text{ (g)}
\]
- Standard electrode potential, \( E^\circ = 0.000 \text{ V} \)
2. The second half-reaction:
\[
\text{Hg}_2\text{Cl}_2 \text{ (s)} + 2 \text{e}^- \rightleftharpoons 2 \text{Hg (l)} + 2 \text{Cl}^- \text{ (aq)}
\]
- Standard electrode potential, \( E^\circ = 0.268 \text{ V} \)
**Explanation of Graph or Diagram:**
- There are no graphs or complex diagrams, just cell notation and a table of half-reactions with standard potentials. The table is key for understanding the redox processes and their feasibility under standard conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fef922cf6-bdce-44cc-8ace-35097c591487%2Fd95d4f7e-1ae5-4601-9652-c4d8945bf59c%2Fic9ti8_processed.png&w=3840&q=75)
Transcribed Image Text:The given image depicts a galvanic cell notation and a table containing standard electrode potentials.
**Galvanic Cell Notation:**
- The cell notation is written as:
\( \text{Pt (s) } \| \text{ H}_2 \text{ (g) (0.85 atm) } \| \text{ RNH}_2 \text{ (aq) (0.10 M), RNH}_3\text{Cl (aq) (0.050 M) } \| \text{ SHE} \).
This notation describes a galvanic cell consisting of:
- A platinum electrode (Pt \((s)\))
- Hydrogen gas (\( \text{H}_2 \)), at a pressure of 0.85 atm
- An aqueous solution containing RNH\(_2\) at 0.10 M and RNH\(_3\)Cl at 0.050 M
- The Standard Hydrogen Electrode (SHE) as the reference
**Table of Half-Reactions:**
- The table presents the electrochemical half-reactions along with their standard electrode potentials \(E^\circ\).
1. The first half-reaction:
\[
2 \text{H}^+ \text{ (aq)} + 2 \text{e}^- \rightleftharpoons \text{H}_2 \text{ (g)}
\]
- Standard electrode potential, \( E^\circ = 0.000 \text{ V} \)
2. The second half-reaction:
\[
\text{Hg}_2\text{Cl}_2 \text{ (s)} + 2 \text{e}^- \rightleftharpoons 2 \text{Hg (l)} + 2 \text{Cl}^- \text{ (aq)}
\]
- Standard electrode potential, \( E^\circ = 0.268 \text{ V} \)
**Explanation of Graph or Diagram:**
- There are no graphs or complex diagrams, just cell notation and a table of half-reactions with standard potentials. The table is key for understanding the redox processes and their feasibility under standard conditions.
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