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Zn (s) Zn + Ni²+ Zn2+ (aq) (aq) → Zn²+ (ay) + Ni (0.112 M) || Ni2+ E = +0.37 V (2.53 M) Ni (5)

Zn (s) Zn + Ni²+ Zn2+ (aq) (aq) → Zn²+ (ay) + Ni (0.112 M) || Ni2+ E = +0.37 V (2.53 M) Ni (5)

Chemistry
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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Given the voltaic cell, what is the cell potential at the non standard conditions given in the cell schematic?
### Galvanic Cell Reaction and Notation #### Chemical Reaction \[ \text{Zn}_{(s)} + \text{Ni}^{2+}_{(aq)} \rightarrow \text{Zn}^{2+}_{(aq)} + \text{Ni}_{(s)} \] - **Zinc (Zn)** in the solid state reacts with **Nickel ions (\( \text{Ni}^{2+} \))** in aqueous solution. - **Zinc ions (\( \text{Zn}^{2+} \))** in aqueous solution are produced, along with solid **Nickel (Ni)**. - The standard cell potential (\( E^\circ \)) for this reaction is \( +0.37 \, \text{V} \). #### Cell Notation \[ \text{Zn}_{(s)} \, | \, \text{Zn}^{2+}_{(aq)} \, (0.112 \, \text{M}) \, || \, \text{Ni}^{2+}_{(aq)} \, (2.53 \, \text{M}) \, | \, \text{Ni}_{(s)} \] - **Anode (Oxidation Half-Cell):** \( \text{Zn}_{(s)} | \text{Zn}^{2+}_{(aq)} (0.112 \, \text{M}) \) - The zinc metal is oxidized to zinc ions, losing electrons. - **Cathode (Reduction Half-Cell):** \( \text{Ni}^{2+}_{(aq)} (2.53 \, \text{M}) | \text{Ni}_{(s)} \) - Nickel ions are reduced to nickel metal, gaining electrons. - The double vertical lines \( || \) represent the salt bridge that allows ions to flow between the two half-cells, completing the circuit. This galvanic cell setup converts chemical energy into electrical energy, with zinc acting as the reducing agent and nickel as the oxidizing agent.
Transcribed Image Text:### Galvanic Cell Reaction and Notation #### Chemical Reaction \[ \text{Zn}_{(s)} + \text{Ni}^{2+}_{(aq)} \rightarrow \text{Zn}^{2+}_{(aq)} + \text{Ni}_{(s)} \] - **Zinc (Zn)** in the solid state reacts with **Nickel ions (\( \text{Ni}^{2+} \))** in aqueous solution. - **Zinc ions (\( \text{Zn}^{2+} \))** in aqueous solution are produced, along with solid **Nickel (Ni)**. - The standard cell potential (\( E^\circ \)) for this reaction is \( +0.37 \, \text{V} \). #### Cell Notation \[ \text{Zn}_{(s)} \, | \, \text{Zn}^{2+}_{(aq)} \, (0.112 \, \text{M}) \, || \, \text{Ni}^{2+}_{(aq)} \, (2.53 \, \text{M}) \, | \, \text{Ni}_{(s)} \] - **Anode (Oxidation Half-Cell):** \( \text{Zn}_{(s)} | \text{Zn}^{2+}_{(aq)} (0.112 \, \text{M}) \) - The zinc metal is oxidized to zinc ions, losing electrons. - **Cathode (Reduction Half-Cell):** \( \text{Ni}^{2+}_{(aq)} (2.53 \, \text{M}) | \text{Ni}_{(s)} \) - Nickel ions are reduced to nickel metal, gaining electrons. - The double vertical lines \( || \) represent the salt bridge that allows ions to flow between the two half-cells, completing the circuit. This galvanic cell setup converts chemical energy into electrical energy, with zinc acting as the reducing agent and nickel as the oxidizing agent.
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