Standard Electrode Potential
The standard reduction potentials of Zn²⁺/Zn and Cu²⁺/Cu electrodes are −0.76 V and +0.34 V respectively. The EMF of a Daniell cell is:
Select the correct option:
Solution
1.10 V
The EMF of a galvanic cell is calculated as E°cell = E°cathode − E°anode. In a Daniell cell, copper acts as the cathode (higher reduction potential) and zinc acts as the anode (lower reduction potential). Therefore, E°cell = (+0.34) − (−0.76) = +0.34 + 0.76 = +1.10 V. A positive cell potential confirms the spontaneity of the overall reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). The magnitude of 1.10 V is a well-known standard value for this electrochemical cell.
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About This Question
- Subject
- chemistry
- Chapter
- redox reactions and electrochemistry
- Topic
- standard electrode potential
- Difficulty
- Easy
- Year
- 2025
Solution
Correct Answer:
1.10 V
The EMF of a galvanic cell is calculated as E°cell = E°cathode − E°anode. In a Daniell cell, copper acts as the cathode (higher reduction potential) and zinc acts as the anode (lower reduction potential). Therefore, E°cell = (+0.34) − (−0.76) = +0.34 + 0.76 = +1.10 V. A positive cell potential confirms the spontaneity of the overall reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). The magnitude of 1.10 V is a well-known standard value for this electrochemical cell.
This easy difficulty chemistry question is from the chapter redox reactions and electrochemistry, covering the topic of standard electrode potential. It appeared in the 2025 exam.
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