The volume at NTP occupied by 11 g of ` CO_(2)` is :

Options

A. 11.2 litre
B. 2.8 litre
C. 5.6 litre
D. 2.24 litre

Explanation

To find the volume at NTP occupied by 11 g of carbon dioxide (CO₂), we can follow these steps:

### Step 1: Determine the molecular weight of CO₂
The molecular weight of carbon dioxide can be calculated by summing the atomic masses of its constituent elements:
- Carbon (C) has an atomic mass of 12 g/mol.
- Oxygen (O) has an atomic mass of 16 g/mol, and since there are two oxygen atoms in CO₂, we multiply by 2.

\[ \text{Molecular weight of CO₂} = 12 + (2 \times 16) = 12 + 32 = 44 \text{ g/mol} \]

### Step 2: Calculate the number of moles of CO₂
Using the formula for the number of moles:

\[ \text{Number of moles} = \frac{\text{Weight of gas}}{\text{Molecular weight}} \]

Given that the weight of CO₂ is 11 g:

\[ \text{Number of moles} = \frac{11 \text{ g}}{44 \text{ g/mol}} = 0.25 \text{ moles} \]

### Step 3: Use the molar volume to find the volume at NTP
At Normal Temperature and Pressure (NTP), the molar volume of any ideal gas is approximately 22.4 liters per mole. Therefore, the volume occupied by the gas can be calculated as:

\[ \text{Volume} = \text{Number of moles} \times \text{Molar volume} \]

Substituting the values we have:

\[ \text{Volume} = 0.25 \text{ moles} \times 22.4 \text{ L/mol} = 5.6 \text{ liters} \]

### Final Answer
The volume at NTP occupied by 11 g of CO₂ is **5.6 liters**.

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