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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Question
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**Calculate \( E_{cell} \) for the redox reaction.**
*(Round to 2 decimal places)*
---
**What is \([Ni^{2+}]\) when \( E_{cell} \) reaches 0.03 V?**
*(Round to 2 significant figures)*
---
(Note: This element describes electrochemical cell calculations typically covered in chemistry courses. \( E_{cell} \) represents the electromotive force of the cell, and \([Ni^{2+}]\) refers to the concentration of nickel(II) ions.)
Additionally, in an educational context, it's beneficial to include explanations or background information on the Nernst equation, redox reactions, and the significance of significant figures in measurements and calculations. This can enable a student to not just solve the problem, but also understand the underlying principles.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F38a9992d-9c05-40da-9474-aaafff450dc4%2Fe000a83e-9674-486c-be7b-29efc3fb07af%2F20len9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:---
**Calculate \( E_{cell} \) for the redox reaction.**
*(Round to 2 decimal places)*
---
**What is \([Ni^{2+}]\) when \( E_{cell} \) reaches 0.03 V?**
*(Round to 2 significant figures)*
---
(Note: This element describes electrochemical cell calculations typically covered in chemistry courses. \( E_{cell} \) represents the electromotive force of the cell, and \([Ni^{2+}]\) refers to the concentration of nickel(II) ions.)
Additionally, in an educational context, it's beneficial to include explanations or background information on the Nernst equation, redox reactions, and the significance of significant figures in measurements and calculations. This can enable a student to not just solve the problem, but also understand the underlying principles.
![### Galvanic Cell Composition: Ni/Ni²⁺ and Co/Co²⁺ Half-Cells
A galvanic cell is comprised of a nickel (Ni/Ni²⁺) half-cell and a cobalt (Co/Co²⁺) half-cell. The initial concentrations and conditions for these half-cells are as follows:
- \([Ni^{2+}] = 0.80 \, M\)
- \([Co^{2+}] = 0.20 \, M\)
- Temperature = \(298.15 \, K\)
The table below provides the standard electrode potentials (E°) of the half-reactions in volts (V).
| **Half-reaction** | **E° (V)** |
|------------------------------|------------|
| \(Ni^{2+}(aq) + 2e^{-} \rightarrow Ni(s)\) | -0.25 |
| \(Co^{2+}(aq) + 2e^{-} \rightarrow Co(s)\) | -0.28 |
#### Explanation of the Table:
1. **Half-reactions**:
- **Nickel half-cell**: \( Ni^{2+}(aq) + 2e^- \rightarrow Ni(s) \)
- **Cobalt half-cell**: \( Co^{2+}(aq) + 2e^- \rightarrow Co(s) \)
2. **Standard Electrode Potentials (E°)**:
- The \(E°\) value for the nickel half-reaction is \(-0.25 \, V\).
- The \(E°\) value for the cobalt half-reaction is \(-0.28 \, V\).
Standard electrode potentials are essential for understanding which half-cell will act as the anode and which will function as the cathode in the galvanic cell. The half-cell with the less negative potential (Ni/Ni²⁺ in this case) will act as the cathode, while the half-cell with the more negative potential (Co/Co²⁺) will act as the anode. The overall cell potential (E° cell) can be calculated for deeper analysis of the electrochemical reactions involved.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F38a9992d-9c05-40da-9474-aaafff450dc4%2Fe000a83e-9674-486c-be7b-29efc3fb07af%2Fx8jb4v_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Galvanic Cell Composition: Ni/Ni²⁺ and Co/Co²⁺ Half-Cells
A galvanic cell is comprised of a nickel (Ni/Ni²⁺) half-cell and a cobalt (Co/Co²⁺) half-cell. The initial concentrations and conditions for these half-cells are as follows:
- \([Ni^{2+}] = 0.80 \, M\)
- \([Co^{2+}] = 0.20 \, M\)
- Temperature = \(298.15 \, K\)
The table below provides the standard electrode potentials (E°) of the half-reactions in volts (V).
| **Half-reaction** | **E° (V)** |
|------------------------------|------------|
| \(Ni^{2+}(aq) + 2e^{-} \rightarrow Ni(s)\) | -0.25 |
| \(Co^{2+}(aq) + 2e^{-} \rightarrow Co(s)\) | -0.28 |
#### Explanation of the Table:
1. **Half-reactions**:
- **Nickel half-cell**: \( Ni^{2+}(aq) + 2e^- \rightarrow Ni(s) \)
- **Cobalt half-cell**: \( Co^{2+}(aq) + 2e^- \rightarrow Co(s) \)
2. **Standard Electrode Potentials (E°)**:
- The \(E°\) value for the nickel half-reaction is \(-0.25 \, V\).
- The \(E°\) value for the cobalt half-reaction is \(-0.28 \, V\).
Standard electrode potentials are essential for understanding which half-cell will act as the anode and which will function as the cathode in the galvanic cell. The half-cell with the less negative potential (Ni/Ni²⁺ in this case) will act as the cathode, while the half-cell with the more negative potential (Co/Co²⁺) will act as the anode. The overall cell potential (E° cell) can be calculated for deeper analysis of the electrochemical reactions involved.
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