Products of electrolysis depend on the nature of material being electrlysed and the type of electrodes being used. If the electrode is inert (e.g., platinum or gold), it does not participate in the chemical reaction and acts only as source or sink for electrons. On the other hand, if the electrode is reactive, it participates in the electrode reaction. thus, the products of electrolysis may be different for reactive and inert electrodes.
Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells.
In these question, a statement of assertion followed by a statement of reason. choose the correct answer out of the following choices.
Q. Assertion (A): The negative sign in the expression `E_(Zn^(2+)//Zn)=-0.76`V means `Zn^(2+)` cannot be oxidised to Zn.
Reason (R): Zn is more reactive than hydrogen & Zn will oxidised, & `H^(+)` will get reduced.

Options

A. Assertion and Reason both are correct statements and reason is correct explanation for assertion.
B. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
C. Assertion is correct statement butreason is wrong statement.
D. Assertion is wrong statement but reason is correct statement.

Explanation

To solve the question, we need to analyze both the assertion and the reason provided in the context of electrochemistry and the reactivity of metals.

### Step-by-Step Solution:

1. **Understanding the Assertion (A)**:
- The assertion states that the negative sign in the expression \( E_{(Zn^{2+}/Zn)} = -0.76 \, V \) means that \( Zn^{2+} \) cannot be oxidized to Zn.
- In electrochemistry, a negative standard electrode potential (\( E^0 \)) indicates that the reduction of the species is non-spontaneous under standard conditions. Therefore, the assertion is correct in stating that \( Zn^{2+} \) cannot be reduced to Zn spontaneously.

2. **Understanding the Reason (R)**:
- The reason states that zinc is more reactive than hydrogen, and thus zinc will oxidize while \( H^+ \) will get reduced.
- This is based on the reactivity series of metals, where zinc is indeed more reactive than hydrogen. Therefore, in the presence of an acid (like HCl), zinc will displace hydrogen and oxidize to \( Zn^{2+} \), while \( H^+ \) ions will get reduced to hydrogen gas (\( H_2 \)). This statement is also correct.

3. **Conclusion**:
- Since both the assertion and the reason are true, and the reason correctly explains the assertion, we can conclude that the answer is option 1 (both A and R are true, and R is the correct explanation for A).

### Final Answer:
The correct answer is option 1: Both Assertion (A) and Reason (R) are true, and R is the correct explanation for A.

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