A galvanic cell can be prepared from copper and tin. Which of the following statements is true? Cu2*(aq) + 2e¯ - → Cu(s) E° = 0.34 V Sn2*(aq) + 2e¯ - Sn(aq) E° = -0.14 V > The mass of copper electrode will increase. Oxidation occurs at the copper electrode O Sn2+ will be reduced to Sn at the tin electrode. O Tin will be produced at the tin electrode
A galvanic cell can be prepared from copper and tin. Which of the following statements is true? Cu2*(aq) + 2e¯ - → Cu(s) E° = 0.34 V Sn2*(aq) + 2e¯ - Sn(aq) E° = -0.14 V > The mass of copper electrode will increase. Oxidation occurs at the copper electrode O Sn2+ will be reduced to Sn at the tin electrode. O Tin will be produced at the tin electrode
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![### Galvanic Cell Formation from Copper and Tin
A galvanic cell can be prepared from copper and tin. The following reactions represent the half-reactions for copper and tin:
#### Copper Reaction:
\[ \text{Cu}^{2+}(aq) + 2\text{e}^- \rightarrow \text{Cu}(s) \]
\[ \text{E}^\circ = 0.34 \, \text{V} \]
#### Tin Reaction:
\[ \text{Sn}^{2+}(aq) + 2\text{e}^- \rightarrow \text{Sn}(aq) \]
\[ \text{E}^\circ = -0.14 \, \text{V} \]
### Question
Which of the following statements is true for the reactions above?
1. The mass of the copper electrode will increase.
2. Oxidation occurs at the copper electrode.
3. \(\text{Sn}^{2+}\) will be reduced to \(\text{Sn}\) at the tin electrode.
4. Tin will be produced at the tin electrode.
### Explanation
In a galvanic cell, the reduction occurs at the electrode with the higher reduction potential. Thus, copper ions will be reduced to copper metal, increasing the mass of the copper electrode. This makes the first statement true.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F69ee2ea2-08ba-468b-bb09-90c697d87fdb%2Fcfc1a71c-1ab7-4ecc-88aa-00b8a29cc6a5%2F7053sxe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Galvanic Cell Formation from Copper and Tin
A galvanic cell can be prepared from copper and tin. The following reactions represent the half-reactions for copper and tin:
#### Copper Reaction:
\[ \text{Cu}^{2+}(aq) + 2\text{e}^- \rightarrow \text{Cu}(s) \]
\[ \text{E}^\circ = 0.34 \, \text{V} \]
#### Tin Reaction:
\[ \text{Sn}^{2+}(aq) + 2\text{e}^- \rightarrow \text{Sn}(aq) \]
\[ \text{E}^\circ = -0.14 \, \text{V} \]
### Question
Which of the following statements is true for the reactions above?
1. The mass of the copper electrode will increase.
2. Oxidation occurs at the copper electrode.
3. \(\text{Sn}^{2+}\) will be reduced to \(\text{Sn}\) at the tin electrode.
4. Tin will be produced at the tin electrode.
### Explanation
In a galvanic cell, the reduction occurs at the electrode with the higher reduction potential. Thus, copper ions will be reduced to copper metal, increasing the mass of the copper electrode. This makes the first statement true.
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