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Assertion : For the Daniel cell, Zn//Zn^...

Assertion : For the Daniel cell, `Zn//Zn^(2+)||Cu^(2+)|Cu" with "E_(cell)=1.1V` results into flow of electron from cathode to anode.
Reason : Zn is deposited at anode and Cu is dissolved at cathode.

A

if both Assertion and Reason are true and reason is the correct explanation of the assertion.

B

if both assertion and reason are true but reason is not the correct expalanation of the assertion

C

if assertion is true, reason is false

D

both assertion and reason are false statements.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question, we need to analyze both the assertion and the reason provided. ### Step 1: Understand the Assertion The assertion states that in a Daniel cell represented as `Zn//Zn^(2+)||Cu^(2+)|Cu`, with an electromotive force (E_cell) of 1.1 V, there is a flow of electrons from the cathode to the anode. **Explanation**: In a Daniel cell, the anode is where oxidation occurs (loss of electrons), and the cathode is where reduction occurs (gain of electrons). In this case, zinc (Zn) is oxidized to zinc ions (Zn²⁺) at the anode, and copper ions (Cu²⁺) are reduced to copper (Cu) at the cathode. Therefore, the flow of electrons is actually from the anode (where zinc is oxidized) to the cathode (where copper is reduced). ### Step 2: Understand the Reason The reason states that zinc is deposited at the anode and copper is dissolved at the cathode. **Explanation**: This statement is incorrect in the context of a functioning Daniel cell. At the anode, zinc does not get deposited; instead, zinc ions go into the solution as zinc is oxidized. Conversely, at the cathode, copper ions from the solution are reduced and deposited as solid copper. Therefore, the correct statement should be that zinc is oxidized at the anode, and copper is deposited at the cathode. ### Step 3: Conclusion Based on the analysis: - The assertion is **incorrect** because it states that electrons flow from cathode to anode, which is not true; they flow from anode to cathode. - The reason is also **incorrect** because it states that zinc is deposited at the anode, which is not the case. Thus, both the assertion and reason are false. ### Final Answer: Both the assertion and reason are false. ---
To solve the question, we need to analyze both the assertion and the reason provided. ### Step 1: Understand the Assertion The assertion states that in a Daniel cell represented as `Zn//Zn^(2+)||Cu^(2+)|Cu`, with an electromotive force (E_cell) of 1.1 V, there is a flow of electrons from the cathode to the anode. **Explanation**: In a Daniel cell, the anode is where oxidation occurs (loss of electrons), and the cathode is where reduction occurs (gain of electrons). In this case, zinc (Zn) is oxidized to zinc ions (Zn²⁺) at the anode, and copper ions (Cu²⁺) are reduced to copper (Cu) at the cathode. Therefore, the flow of electrons is actually from the anode (where zinc is oxidized) to the cathode (where copper is reduced). ...
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