(b) What would be the molar mass of a compound if 6.21 g of it dissolved in 24.0 g of chloroform form a solution that has a boiling point of `68.04^(@)C`. The boiling point of pure chloroform is `61.7^(@)C` and the boiling point elevation constant `K_(b)` for chloroform is `3.63^(@)C//m`.

Explanation

To find the molar mass of the compound, we can follow these steps:

### Step 1: Calculate the change in boiling point (ΔT_b)
The change in boiling point is calculated using the formula:
\[ \Delta T_b = T_{solution} - T_{pure\ solvent} \]
Where:
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