`1.0 g` of non-electrolyte solute dissolved in `50.0 g` of benzene lowered the freezing point of benzene by `0.40 K`. The freezing point depression constant of benzene is `5.12 kg mol^(-1)`. Find the molecular mass of the solute.

Explanation

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

\[ \Delta T_F = K_F \times m \]

Where:
- \(\Delta T_F\) = freezing point depression (in Kelvin)
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