A flask of capacity 2 L is heated from `35 C^(@)` to `45 C^(@)`. What volume of air will escape from the flask ?

Options

A. 10 mL
B. 20 mL
C. 60 mL
D. 50 mL

Explanation

To solve the problem of how much air will escape from a flask when it is heated from 35°C to 45°C, we can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature (in Kelvin) when pressure is held constant.

### Step-by-Step Solution:

1. **Identify Given Values:**
- Initial volume (V1) = 2 L
- Initial temperature (T1) = 35°C
- Final temperature (T2) = 45°C

2. **Convert Temperatures to Kelvin:**
- To convert Celsius to Kelvin, use the formula:
\[ K = °C + 273 \]
- For T1:
\[ T1 = 35 + 273 = 308 \, K \]
- For T2:
\[ T2 = 45 + 273 = 318 \, K \]

3. **Apply Charles's Law:**
- According to Charles's Law:
\[ \frac{V1}{T1} = \frac{V2}{T2} \]
- Rearranging to find V2:
\[ V2 = \frac{V1 \times T2}{T1} \]

4. **Substitute the Values:**
- Plugging in the values:
\[ V2 = \frac{2 \, L \times 318 \, K}{308 \, K} \]

5. **Calculate V2:**
- Performing the calculation:
\[ V2 = \frac{636}{308} \approx 2.06 \, L \]

6. **Determine the Volume of Air Escaped:**
- The volume of air that escapes is the difference between V2 and V1:
\[ \text{Volume of air escaped} = V2 - V1 = 2.06 \, L - 2 \, L = 0.06 \, L \]
- Converting to milliliters:
\[ 0.06 \, L = 60 \, mL \]

### Final Answer:
The volume of air that will escape from the flask is **60 mL**.