The vapour pressure of water at `25^(@)C` is 18 mmHg. If 18 g of glucose`(C_(6)H_(12)O_(6))` is added to 178.2 g of water at `20^(@)C`, the vapour pressure of the resulting solution will be :

Options

A. 17.70 mmHg
B. 15.750 mmHg
C. 16.500 mmHg
D. 17.82 mmHg

Explanation

To solve the problem of finding the vapor pressure of the resulting solution when 18 g of glucose is added to 178.2 g of water, we will use Raoult's Law. Here’s a step-by-step breakdown of the solution:

### Step 1: Determine the Molar Mass of Glucose
The formula for glucose is \( C_6H_{12}O_6 \).
- The molar mass of glucose can be calculated as follows:
- Carbon (C): \( 6 \times 12 \, \text{g/mol} = 72 \, \text{g/mol} \)
- Hydrogen (H): \( 12 \times 1 \, \text{g/mol} = 12 \, \text{g/mol} \)
- Oxygen (O): \( 6 \times 16 \, \text{g/mol} = 96 \, \text{g/mol} \)
...