If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter? Half-Reaction Zn2+ E (V) Zn(s) -0.76 (aq) + 2e Ag (aq) + e Ag(s) +0.80 - %media:chapter18_40.jpg% -
If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter? Half-Reaction Zn2+ E (V) Zn(s) -0.76 (aq) + 2e Ag (aq) + e Ag(s) +0.80 - %media:chapter18_40.jpg% -
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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![Title: Calculating Voltage in an Electrochemical Cell
**Problem Statement:**
If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter?
**Half-Reaction | \( E^\circ \) (V)**
\[ \text{Zn}^{2+} (aq) + 2e^- \rightarrow \text{Zn}(s) \quad -0.76 \, \text{V} \]
\[ \text{Ag}^{+} (aq) + e^- \rightarrow \text{Ag}(s) \quad +0.80 \, \text{V} \]
**Explanation:**
In this example, the electrochemical cell is constructed using the zinc and silver half-reactions. The standard electrode potentials (\( E^\circ \)) for each of these half-reactions are provided. To calculate the overall voltage measured, you need to find the difference between the standard reduction potentials of the cathode and anode:
1. **Determine the cathode and anode:**
- The half-reaction with the more positive \( E^\circ \) value is the reduction reaction at the cathode. In this case, it is the silver reaction.
- The half-reaction with the less positive (or more negative) \( E^\circ \) value is the oxidation reaction at the anode. Here, it is the zinc reaction.
2. **Calculate the cell potential (\( E_{\text{cell}}^\circ \)):**
\[
E_{\text{cell}}^\circ = E_{\text{cathode}}^\circ - E_{\text{anode}}^\circ
\]
\[
E_{\text{cell}}^\circ = 0.80 \, \text{V} - (-0.76 \, \text{V}) = 0.80 \, \text{V} + 0.76 \, \text{V} = 1.56 \, \text{V}
\]
**Conclusion:**
The voltage measured on the voltmeter for this electrochemical cell will be \( 1.56 \, \text{V} \). This calculated voltage represents the maximum potential difference that the cell can produce under standard conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ceb2d65-29b4-49d4-9830-4ba06589987b%2F94ce4b26-a4f9-4373-a482-bfb6865d5e1a%2F9vvy2ks_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Title: Calculating Voltage in an Electrochemical Cell
**Problem Statement:**
If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter?
**Half-Reaction | \( E^\circ \) (V)**
\[ \text{Zn}^{2+} (aq) + 2e^- \rightarrow \text{Zn}(s) \quad -0.76 \, \text{V} \]
\[ \text{Ag}^{+} (aq) + e^- \rightarrow \text{Ag}(s) \quad +0.80 \, \text{V} \]
**Explanation:**
In this example, the electrochemical cell is constructed using the zinc and silver half-reactions. The standard electrode potentials (\( E^\circ \)) for each of these half-reactions are provided. To calculate the overall voltage measured, you need to find the difference between the standard reduction potentials of the cathode and anode:
1. **Determine the cathode and anode:**
- The half-reaction with the more positive \( E^\circ \) value is the reduction reaction at the cathode. In this case, it is the silver reaction.
- The half-reaction with the less positive (or more negative) \( E^\circ \) value is the oxidation reaction at the anode. Here, it is the zinc reaction.
2. **Calculate the cell potential (\( E_{\text{cell}}^\circ \)):**
\[
E_{\text{cell}}^\circ = E_{\text{cathode}}^\circ - E_{\text{anode}}^\circ
\]
\[
E_{\text{cell}}^\circ = 0.80 \, \text{V} - (-0.76 \, \text{V}) = 0.80 \, \text{V} + 0.76 \, \text{V} = 1.56 \, \text{V}
\]
**Conclusion:**
The voltage measured on the voltmeter for this electrochemical cell will be \( 1.56 \, \text{V} \). This calculated voltage represents the maximum potential difference that the cell can produce under standard conditions.
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