1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. The freezing point depression constant of benzene is `"5.12 K kg mol"^(-1)`. Find the molar mass of solute.

Explanation

To find the molar mass of the non-electrolyte solute, we can use the formula for freezing point depression:

\[ \Delta T_f = K_f \cdot m \]

where:
- \(\Delta T_f\) is the freezing point depression,
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