If 1.2 g of a metal displaces 1.12 litre of hydrogen at NTP. Equivalent mass of the metal would be -

Options

A. `1.2xx11.2`
B. 12
C. 24
D. `1.2+11.2`

Explanation

To find the equivalent mass of the metal that displaces 1.12 liters of hydrogen gas at Normal Temperature and Pressure (NTP), we can follow these steps:

### Step-by-Step Solution:

1. **Understand the displacement of hydrogen**: At NTP, 1 mole of any gas occupies 22.4 liters. Therefore, 1 mole of hydrogen (H₂) will also occupy 22.4 liters. Since hydrogen is diatomic, its molar volume is 22.4 L.

2. **Calculate the number of moles of hydrogen displaced**:
\[ \text{Moles of H}_2 = \frac{\text{Volume of H}_2}{\text{Molar Volume at NTP}} = \frac{1.12 \, \text{L}}{22.4 \, \text{L/mol}} = 0.05 \, \text{mol} \]

3. **Determine the equivalent weight of the metal**: The equivalent weight of a metal can be calculated using the formula:
\[ \text{Equivalent weight} = \frac{\text{Weight of the metal}}{\text{Moles of H}_2} \]
Here, the weight of the metal is given as 1.2 g.

4. **Substitute the values into the formula**:
\[ \text{Equivalent weight} = \frac{1.2 \, \text{g}}{0.05 \, \text{mol}} = 24 \, \text{g/equiv} \]

5. **Final Result**: The equivalent mass of the metal is 24 g/equiv.

### Summary of Calculation:
- Weight of metal = 1.2 g
- Volume of hydrogen = 1.12 L
- Moles of hydrogen = 0.05 mol
- Equivalent mass of the metal = 24 g/equiv