An aqueous solution of glucose is made by dissolving 10 g of glucose in 90 g water at 303 K. If the V.P. of pure water at 303 K be 32.8 mm Hg, what would be V.P. of the solution ?

Explanation

To find the vapor pressure of the glucose solution, we will use Raoult's Law, which states that the vapor pressure of a solution (P_S) is related to the vapor pressure of the pure solvent (P_0) and the mole fraction of the solute. Here’s a step-by-step solution:

### Step 1: Calculate the number of moles of glucose and water

1. **Calculate moles of glucose**:
- Given mass of glucose = 10 g
- Molar mass of glucose (C₆H₁₂O₆) = 180 g/mol
- Moles of glucose = mass / molar mass = 10 g / 180 g/mol = 0.0556 mol
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