Statement-I: If an aqueous solution of `NaCI` is electrolysed, the product obtained at the cathode is `H_(2)` gas and no Na.
Because Statement-II: Gases are liberated faster than the metals.

Answer

To solve the question regarding the electrolysis of an aqueous solution of NaCl, we will analyze both statements provided and determine their validity step by step.

### Step 1: Understanding Electrolysis of NaCl Solution
When an aqueous solution of NaCl is electrolyzed, it dissociates into its constituent ions:
\[ \text{NaCl} \rightarrow \text{Na}^+ + \text{Cl}^- \]

### Step 2: Identifying Products at the Electrodes
During electrolysis, the following reactions can occur at the electrodes:
- At the cathode (negative electrode), reduction occurs. The possible reduction reactions are:
- \( \text{Na}^+ + e^- \rightarrow \text{Na} \) (sodium metal)
- \( 2 \text{H}_2\text{O} + 2 e^- \rightarrow \text{H}_2 + 2 \text{OH}^- \) (hydrogen gas)

- At the anode (positive electrode), oxidation occurs. The possible oxidation reactions are:
- \( 2 \text{Cl}^- \rightarrow \text{Cl}_2 + 2 e^- \) (chlorine gas)
- \( 2 \text{OH}^- \rightarrow \text{O}_2 + 2 \text{H}^+ + 4 e^- \) (oxygen gas)

### Step 3: Analyzing Statement-I
**Statement-I:** "If an aqueous solution of NaCl is electrolyzed, the product obtained at the cathode is H₂ gas and no Na."

From our analysis, at the cathode, the reduction of water to form hydrogen gas is favored over the reduction of sodium ions to form sodium metal. This is because the standard reduction potential for the formation of hydrogen gas from water is more favorable than that for sodium ions. Therefore, Statement-I is **True**.

### Step 4: Analyzing Statement-II
**Statement-II:** "Gases are liberated faster than the metals."

This statement can be understood in the context of electrolysis. Gases like hydrogen and chlorine are produced at the electrodes during the electrolysis of NaCl solution. The liberation of gas occurs at a faster rate than the deposition of metals because gas bubbles can escape immediately, while metals require time to deposit on the electrode surface. Thus, Statement-II is also **True**.

### Conclusion
Both statements are true:
- Statement-I is true because hydrogen gas is produced at the cathode instead of sodium metal.
- Statement-II is true because gases are liberated faster than metals during electrolysis.

### Final Answer
Both Statement-I and Statement-II are true.

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