During the electrolysis of water 4 mol of electrons were transferred from anode to cathode. The total volume of gases produced at STP will be approximately

Options

A. 67.2L
B. 22.4L
C. 44.8L
D. 89.4L

Answer

To solve the problem of determining the total volume of gases produced during the electrolysis of water when 4 moles of electrons are transferred, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reactions**:
- At the anode (oxidation), the half-reaction is:
\[ 4 \text{OH}^- \rightarrow 2 \text{H}_2\text{O} + \text{O}_2 + 4 \text{e}^- \]
- At the cathode (reduction), the half-reaction is:
\[ 4 \text{H}_2\text{O} + 4 \text{e}^- \rightarrow 2 \text{H}_2 + 4 \text{OH}^- \]

2. **Combine the Half-Reactions**:
- The overall reaction for the electrolysis of water can be written as:
\[ 2 \text{H}_2\text{O} \rightarrow 2 \text{H}_2 + \text{O}_2 \]

3. **Determine Moles of Gases Produced**:
- From the balanced equation, we see that:
- 2 moles of water produce 2 moles of hydrogen gas (\( \text{H}_2 \)) and 1 mole of oxygen gas (\( \text{O}_2 \)).
- Therefore, the total moles of gas produced = \( 2 \text{ moles of } H_2 + 1 \text{ mole of } O_2 = 3 \text{ moles of gas} \).

4. **Calculate Volume at STP**:
- At Standard Temperature and Pressure (STP), 1 mole of gas occupies 22.4 liters.
- Thus, the total volume of gas produced from 3 moles is:
\[ 3 \text{ moles} \times 22.4 \text{ L/mole} = 67.2 \text{ L} \]

5. **Final Answer**:
- Therefore, the total volume of gases produced during the electrolysis of water when 4 moles of electrons are transferred is approximately **67.2 liters**.