The molar volume of CO2 at NTP is :

Explanation

To find the molar volume of CO2 at Normal Temperature and Pressure (NTP), we can use the Ideal Gas Law, which is expressed as:

\[ PV = nRT \]

Where:
- \( P \) = Pressure
- \( V \) = Volume
- \( n \) = Number of moles
- \( R \) = Ideal gas constant
- \( T \) = Temperature in Kelvin

### Step-by-Step Solution:

1. **Identify the conditions for NTP**:
- Normal Temperature (T) = 273 K (0°C)
- Normal Pressure (P) = 1 atm

2. **Use the Ideal Gas Law**:
- We need to find the volume (V) for 1 mole of gas (n = 1).
- Rearranging the Ideal Gas Law gives us:
\[ V = \frac{nRT}{P} \]

3. **Substitute the values**:
- For 1 mole of CO2, we have:
- \( n = 1 \)
- \( R = 0.0821 \, \text{L atm K}^{-1} \text{mol}^{-1} \) (Ideal gas constant)
- \( T = 273 \, \text{K} \)
- \( P = 1 \, \text{atm} \)

- Plugging in these values:
\[ V = \frac{1 \times 0.0821 \times 273}{1} \]

4. **Calculate the volume**:
- Performing the calculation:
\[ V = 0.0821 \times 273 = 22.4133 \, \text{L} \]

5. **Round off the answer**:
- The molar volume of CO2 at NTP is approximately:
\[ V \approx 22.4 \, \text{L} \]

### Final Answer:
The molar volume of CO2 at NTP is **22.4 liters**.

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