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Calculate the molal depression constant ...

Calculate the molal depression constant of a solvent which has freezing point `16.6^(@)C` and latent heat of fusion `180.75 "J g"^(-1)` :

A

`2.68`

B

`3.86`

C

`4.68`

D

`2.86`

Text Solution

Verified by Experts

The correct Answer is:
B
`K_(f)=(RT_(f)^(2))/(1000xx L_(f)), R=8.314 JK^(-1)mol^(-1)`
`T_(f)=273+16.6=289.6K , L_(f)=180.75 Jg^(-1)`
`K_(f)=(8.314xx289.6xx289.6)/(1000xx180.75)=3.86`
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Knowledge Check

  • Statement - I. Greater the molal depression constant of the solvent used less in the freezing point of the solution. Statement - II. Depression in freezing point depends upon the nature of the solvent.

    A
    Statement-1 is true, statement-2 is true and statement-2 is correct explanation for statement-1.
    B
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    C
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    D
    Statement-1 is false, statement-2 is true.

  • The molal depression constant for a solvent is 4.9. The depression in freezing point for a millimolal solution of a non-electrolyte in the solvent is

    A
    0.49
    B
    4.9
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    D
    0.0049.

  • Molal depression constant for solvent is 30 K. kg " mol"^(-1) The depression in the freezing point of the solvent for 0.04 mol Kg^(-1) solution of N_2SO_4 is :(Assume complete dissociations of the electrolyte)

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