Assertion `(A):` The electrolysis of `NaCl` solution gives `H_(2)(g)` at cathode and `Cl_(2)(g)` at anode.
Reason `(R) : Cl_(2)` has higher oxidation potential than `H_(2)O`

Options

A. If both `(A)` and `(R)` are correct, and `(R)` is the correct explanation of `(A)`.
B. If both `(A)` and `(R)` are correct, but `(R)` is not the correct explanation of `(A)`.
C. If `(A)` is correct, but `(R)` is incorrect.
D. If `(A)` is incorrect, `(R)` is correct.

Explanation

To solve the question regarding the electrolysis of NaCl solution and the assertion and reason provided, we can break it down into a step-by-step analysis.

### Step 1: Understanding the Electrolysis Process
Electrolysis involves the breakdown of a compound in solution using an electric current. In the case of NaCl (sodium chloride) dissolved in water, the solution contains the following ions:
- Sodium ions (Na⁺)
- Chloride ions (Cl⁻)
- Hydrogen ions (H⁺)
- Hydroxide ions (OH⁻)

### Step 2: Identifying the Cathode Reaction
At the cathode, reduction occurs. The species that can be reduced are H⁺ and Na⁺. The reduction potential for H⁺ to H₂ is higher than that for Na⁺ to Na. Therefore, H⁺ will be reduced to form hydrogen gas (H₂):
\[ 2H^+ + 2e^- \rightarrow H_2(g) \]
Thus, hydrogen gas is produced at the cathode.

### Step 3: Identifying the Anode Reaction
At the anode, oxidation occurs. The species that can be oxidized are Cl⁻ and OH⁻. Chloride ions (Cl⁻) can be oxidized to form chlorine gas (Cl₂), while hydroxide ions (OH⁻) can lead to the formation of oxygen gas (O₂). However, Cl⁻ has a higher tendency to be oxidized compared to OH⁻ under standard conditions, leading to the formation of chlorine gas:
\[ 2Cl^- \rightarrow Cl_2(g) + 2e^- \]
Thus, chlorine gas is produced at the anode.

### Step 4: Evaluating the Assertion and Reason
- **Assertion (A)**: The electrolysis of NaCl solution gives H₂(g) at the cathode and Cl₂(g) at the anode. This statement is **correct** based on the reactions identified.
- **Reason (R)**: Cl₂ has a higher oxidation potential than H₂O. This statement is **incorrect**. In fact, Cl₂ has a lower oxidation potential compared to the oxidation of water.

### Conclusion
The assertion is correct, while the reason is incorrect. Therefore, the correct answer is:
**Assertion is correct, reason is incorrect.**

### Final Answer
**Option C: Assertion is correct, Reason is incorrect.**

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