2L of `SO_(2)` gas at 760 mm Hg are transferred to 10 L flask containing oxygen at a particular temperature, the partial pressure of `SO_(2)` in the flask is

Options

A. 63.33 mmHg
B. 152 mmHg
C. 760 mmHg
D. 1330 mmHg

Answer

To solve the problem of finding the partial pressure of SO₂ gas after it is transferred to a 10 L flask, we will use Boyle's Law, which states that for a given mass of gas at constant temperature, the product of pressure and volume is constant (P₁V₁ = P₂V₂).

### Step-by-Step Solution:

1. **Identify the Given Values**:
- Initial volume of SO₂ (V₁) = 2 L
- Initial pressure of SO₂ (P₁) = 760 mm Hg
- Final volume of the flask (V₂) = 10 L

2. **Convert Pressure to Atmospheres (if necessary)**:
- Since we are working with pressures, we can convert 760 mm Hg to atmospheres for easier calculations:
\[ P₁ = \frac{760 \text{ mm Hg}}{760} = 1 \text{ atm} \]

3. **Apply Boyle's Law**:
- According to Boyle's Law:
\[ P₁V₁ = P₂V₂ \]
- Substitute the known values into the equation:
\[ (1 \text{ atm})(2 \text{ L}) = P₂(10 \text{ L}) \]

4. **Solve for P₂**:
- Rearranging the equation to solve for P₂:
\[ P₂ = \frac{(1 \text{ atm})(2 \text{ L})}{10 \text{ L}} = \frac{2}{10} \text{ atm} = 0.2 \text{ atm} \]

5. **Convert P₂ back to mm Hg**:
- To convert the pressure back to mm Hg:
\[ P₂ = 0.2 \text{ atm} \times 760 \text{ mm Hg/atm} = 152 \text{ mm Hg} \]

### Final Answer:
The partial pressure of SO₂ in the flask is **152 mm Hg**.