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Calculatate the mass of compound (molar ...

Calculatate the mass of compound (molar mass = `256 g mol^(-1)` be the dissolved in 75 g of benzene to lower its freezing point by ` 0 .48 k(k_(f) = 5. 12 k kg mol ^(-1)` .

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To solve the problem, we need to calculate the mass of a compound that will lower the freezing point of benzene by 0.48 K. We will use the formula for depression of freezing point, which is given by: \[ \Delta T_f = K_f \cdot m \] Where: - \(\Delta T_f\) = depression in freezing point (0.48 K) ...
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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 K_(f) of benzene is 5.12 K kg mol^(–1) , the freezing point of benzene will be lowered by:-

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 K_(f) of benzene is 5.12 K kg mol^(–1) , the freezing point of benzene will be lowered by:-

Knowledge Check

  • If 1 g of solute (molar mass = 50 g mol^(-1) ) is dissolved in 50 g of solvent and the elevation in boiling point is 1 K. The molar boiling constant of the solvent is

    A
    2
    B
    3
    C
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    D
    5

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