Electrolysis of aqueous HCl solution produces-

Options

A. `H_(2)` gas at the anode
B. `H_(2)` gas at the cathode
C. `Cl_(2)` gas at the cathode
D. `Cl_(2)` and `O_(2)` gases both at the anode

Explanation

To solve the question regarding the electrolysis of aqueous HCl solution, we can break it down into several steps:

### Step-by-Step Solution:

1. **Understanding Electrolysis**: Electrolysis involves passing an electric current through a solution to cause a chemical change. In this case, we are looking at the electrolysis of an aqueous solution of hydrochloric acid (HCl).

2. **Identifying the Components**: In an aqueous solution of HCl, we have H⁺ ions and Cl⁻ ions. When electrolysis occurs, these ions will migrate to the electrodes.

3. **Electrolysis at the Cathode**: The cathode is the negative electrode where reduction occurs. In the case of HCl, the H⁺ ions will move towards the cathode. The reduction half-reaction at the cathode can be represented as:
\[ 2H^+ + 2e^- \rightarrow H_2(g) \]
This means that hydrogen gas (H₂) is produced at the cathode.

4. **Electrolysis at the Anode**: The anode is the positive electrode where oxidation occurs. In the case of HCl, the Cl⁻ ions will move towards the anode. The oxidation half-reaction at the anode can be represented as:
\[ 2Cl^- \rightarrow Cl_2(g) + 2e^- \]
This means that chlorine gas (Cl₂) is produced at the anode.

5. **Final Products**: From the above reactions, we can conclude that during the electrolysis of aqueous HCl, hydrogen gas (H₂) is produced at the cathode and chlorine gas (Cl₂) is produced at the anode.

6. **Conclusion**: Therefore, the products of the electrolysis of aqueous HCl solution are hydrogen gas at the cathode and chlorine gas at the anode.

### Answer:
The electrolysis of aqueous HCl solution produces hydrogen gas (H₂) at the cathode and chlorine gas (Cl₂) at the anode.