1.00 g of non-eletrolyte solute (molar mass 250 g mol − 1 ) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K f of benzene is 5.12 K kg mol − 1 , the freezing point of

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1.00 g of non-eletrolyte solute (molar mass 250 g mol − 1 ) was dissolved in 51.2 g of benzene. If the freezing point depression constant, K f ​ of benzene is 5.12 K kg mol − 1 , the freezing point of benzene will be lowered by:NEET 2006

TestHub · Accepted Answer

Molality of a non-electrolyte solute Δ T f ​ ​ weight of solvent in kg molecular weight of solute weight of solute in gram ​ ​ = 0.0512 250 1 ​ ​ = 250 × 0.0512 1 ​ = 0.0781 m = k f ​ × molality of solution = 5.12 × 0.0781 = 0.4 K ​

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