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  4. 1.00 g of a non-electrolyte solute (molar mass 250g mol-1) was dissolved in 51.2 g of benzene. If the freezing point depression constant, Kf of benzene is 5.12 K kg mol-1, the freezing point of benzene will be lowered by :

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Q. 1.00 g of a non-electrolyte solute (molar mass 250g mol-1) was dissolved in 51.2 g of benzene. If the freezing point depression constant, Kf of benzene is 5.12 K kg mol-1, the freezing point of benzene will be lowered by :

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Solution:

$\Delta T _{ f }-\text { molality } \times K _{ f } $

$\Delta T _{ f }=\left(\frac{1 \times 1000}{250 \times 51.2}\right) \times 5.12$

$\Delta T _{ f }=0.4 \,K$