A certain sample of gas has a volume of `0.2` litre measured at `1 atm` pressure and `0^(@)C`. At the same pressure but at `273^(@)C`, its volume will be

Options

A. 0.4 litre
B. 0.8 litre
C. 27.8 litres
D. 55.6 litres

Explanation

To solve the problem of finding the volume of a gas at a different temperature while keeping the pressure constant, we can use Charles's Law. Charles's Law states that the volume of a gas is directly proportional to its absolute temperature (in Kelvin) when the pressure is held constant.

### Step-by-Step Solution:

1. **Identify Given Values:**
- Initial volume (V1) = 0.2 L
- Initial temperature (T1) = 0°C = 273 K (convert Celsius to Kelvin by adding 273)
- Final temperature (T2) = 273°C = 546 K (convert Celsius to Kelvin)

2. **Use Charles's Law:**
- According to Charles's Law:
\[ \frac{V_2}{V_1} = \frac{T_2}{T_1} \]
- Rearranging gives us:
\[ V_2 = V_1 \times \frac{T_2}{T_1} \]

3. **Substitute the Known Values:**
- Substitute V1, T1, and T2 into the equation:
\[ V_2 = 0.2 \, \text{L} \times \frac{546 \, \text{K}}{273 \, \text{K}} \]

4. **Calculate the Ratio:**
- Calculate the ratio:
\[ \frac{546}{273} = 2 \]

5. **Calculate Final Volume (V2):**
- Now substitute this ratio back into the equation:
\[ V_2 = 0.2 \, \text{L} \times 2 = 0.4 \, \text{L} \]

6. **Conclusion:**
- The final volume of the gas at 273°C and 1 atm pressure is **0.4 L**.

### Final Answer:
The volume of the gas at 273°C and 1 atm pressure will be **0.4 L**.