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

Explanation

To find the molar mass of the compound, we will use the boiling point elevation formula. Here’s a step-by-step solution:

### Step 1: Calculate the boiling point elevation (ΔT_b)
The boiling point elevation (ΔT_b) is given by the difference between the boiling point of the solution and the boiling point of the pure solvent (chloroform).

\[ \Delta T_b = T_{b, \text{solution}} - T_{b, \text{pure solvent}} \]
...