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$1.00 \mathrm{~g}$ of a non-electrolyte solute (molar mass $\left.250 \mathrm{~g} \mathrm{~mol}^{-1}\right)$ was dissolved in $51.2 \mathrm{~g}$ of benzene. If the freezing point depression constant, $\mathrm{K}_{\mathrm{f}}$ of benzene is $5.12 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$, the freezing point of benzene will be lowered by
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$0.4 \mathrm{~K}$
$\Delta \mathrm{T}_{\mathrm{f}}=\mathrm{K}_{\mathrm{f}} \mathrm{m}=5.12 \times \frac{1}{250} \times \frac{1000}{51.2}=0.4 \mathrm{~K}$
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