STATEMENT-1 : Equivalent volume of `H_(2)` is 11.2 L at 1 atm and 273 K.
STATEMENT-2 : `1//2`mole `H_(2)` has produced when 1 mole of `H^(+)` (aq) accepted 1 mole of `e^(-)`.

Options

A. If both the statement are TRUE and STATEMENT -2 is the correct explanation of STATEMENT-1
B. If both the statement are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT- is 1 TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the given question, we will analyze both statements step by step.

### Step 1: Understanding Statement 1
**Statement 1:** Equivalent volume of \( H_2 \) is 11.2 L at 1 atm and 273 K.

- At standard temperature and pressure (STP), the molar volume of any ideal gas is 22.4 L.
- The equivalent volume can be calculated using the formula:
\[ \text{Equivalent Volume} = \frac{\text{Molar Volume}}{n \text{-factor}} \]
- For \( H_2 \), it is produced from the reduction of \( H^+ \) ions. The reaction can be represented as:
\[ 2H^+ + 2e^- \rightarrow H_2 \]
- Here, \( n \)-factor for \( H_2 \) is 2 because 2 moles of electrons are required to produce 1 mole of \( H_2 \).

### Step 2: Calculating Equivalent Volume
- Now substituting the values into the equivalent volume formula:
\[ \text{Equivalent Volume} = \frac{22.4 \, \text{L}}{2} = 11.2 \, \text{L} \]
- Therefore, Statement 1 is **true**.

### Step 3: Understanding Statement 2
**Statement 2:** \( \frac{1}{2} \) mole of \( H_2 \) is produced when 1 mole of \( H^+ \) accepts 1 mole of \( e^- \).

- From the reaction \( 2H^+ + 2e^- \rightarrow H_2 \), we see that:
- 2 moles of \( H^+ \) produce 1 mole of \( H_2 \).
- If 1 mole of \( H^+ \) accepts 1 mole of \( e^- \), it will produce:
\[ \text{Moles of } H_2 = \frac{1 \, \text{mole of } H^+}{2} = \frac{1}{2} \, \text{mole of } H_2 \]
- Thus, Statement 2 is also **true**.

### Step 4: Conclusion
- Since both statements are true and Statement 2 correctly explains Statement 1, the final conclusion is that both statements are true, and Statement 2 is the correct explanation for Statement 1.

### Final Answer
Both statements are true, and Statement 2 is the correct explanation for Statement 1.

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