The volume of 1.0 g of hydrogen in litres at N.T.P. is

Options

A. `2.24`
B. `22.4`
C. `1.12`
D. `11.2`

Explanation

To find the volume of 1.0 g of hydrogen gas (H₂) at Normal Temperature and Pressure (N.T.P.), we can follow these steps:

### Step 1: Understand the Molar Mass of Hydrogen
The molar mass of hydrogen gas (H₂) is approximately 2 grams per mole. This is because each hydrogen atom has a mass of about 1 gram/mole, and there are two hydrogen atoms in a molecule of hydrogen gas.

### Step 2: Use the Molar Volume at N.T.P.
At N.T.P (Normal Temperature and Pressure), 1 mole of any ideal gas occupies a volume of 22.4 liters.

### Step 3: Calculate the Volume for 1 Gram of Hydrogen
Since the molar mass of hydrogen gas is 2 grams, we can determine how much volume 1 gram of hydrogen gas would occupy.

1. Calculate the number of moles in 1 gram of hydrogen:
\[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} = \frac{1 \text{ g}}{2 \text{ g/mol}} = 0.5 \text{ moles} \]

2. Now, calculate the volume occupied by 0.5 moles of hydrogen gas at N.T.P:
\[ \text{Volume} = \text{Number of moles} \times \text{Molar volume} = 0.5 \text{ moles} \times 22.4 \text{ L/mol} = 11.2 \text{ liters} \]

### Conclusion
The volume of 1.0 g of hydrogen gas at N.T.P is **11.2 liters**.

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