Question:
The wrong statement regarding Galvanic cell is
The wrong statement regarding Galvanic cell is
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In a galvanic cell, anode is negative and cathode is positive. In an electrolytic cell, the signs are reversed.
Updated On: May 7, 2026
- In this spontaneous redox reaction occurs
- Salt bridge maintains electrical neutrality between the two solutions
- Anode is represented by \((+)\) and cathode by \((-)\)
- At anode oxidation occurs
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The Correct Option is C
Solution and Explanation
Concept:
A galvanic cell converts chemical energy into electrical energy through a spontaneous redox reaction.
Step 1: In a galvanic cell, the redox reaction is spontaneous.
So statement (A) is correct.
Step 2: The salt bridge allows movement of ions and maintains electrical neutrality between the two half-cells.
So statement (B) is also correct.
Step 3: Oxidation always occurs at the anode.
So statement (D) is correct.
Step 4: In a galvanic cell: \[ \text{Anode is negative} \] and \[ \text{Cathode is positive} \] But the given statement says: \[ \text{Anode is }(+)\text{ and cathode is }(-) \] This is incorrect for a galvanic cell. Therefore, the wrong statement is: \[ \boxed{\text{Anode is represented by }(+)\text{ and cathode by }(-)} \]
Step 1: In a galvanic cell, the redox reaction is spontaneous.
So statement (A) is correct.
Step 2: The salt bridge allows movement of ions and maintains electrical neutrality between the two half-cells.
So statement (B) is also correct.
Step 3: Oxidation always occurs at the anode.
So statement (D) is correct.
Step 4: In a galvanic cell: \[ \text{Anode is negative} \] and \[ \text{Cathode is positive} \] But the given statement says: \[ \text{Anode is }(+)\text{ and cathode is }(-) \] This is incorrect for a galvanic cell. Therefore, the wrong statement is: \[ \boxed{\text{Anode is represented by }(+)\text{ and cathode by }(-)} \]
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