`5g` of compound `A` was dissolved in `100g` of water at `303K`. The vapour pressure of the solution was found to be `4.16` kilopascal. If the vapour pressure of pure water is `4.24 kPa` at this temperature, what is the molecular mass of `A`?

Explanation

To determine the molecular mass of compound A, we will use Raoult's law, which relates the vapor pressure of a solution to the concentration of the solute.

### Step-by-Step Solution:

1. **Identify the given values:**
- Mass of solute (A), \( W_2 = 5 \, \text{g} \)
- Mass of solvent (water), \( W_1 = 100 \, \text{g} \)
- Vapor pressure of the solution, \( P = 4.16 \, \text{kPa} \)
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