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The boiling a point of benzene is 353.23...

The boiling a point of benzene is 353.23K. When 1.80 g of a non-volatile solute was dissolved in 90 g of benzene, the boiling point is raised to 354.11 K. Calculate the molar mass of the solute. `K_(b)` for benzene is 2.53 K kg `mol^(-1)`.

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To calculate the molar mass of the non-volatile solute dissolved in benzene, we can follow these steps: ### Step 1: Calculate the change in boiling point (ΔT_b) The change in boiling point (ΔT_b) is given by the formula: \[ \Delta T_b = T_b - T_{b0} \] Where: ...
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When 10 of a non-volatile solute is dissolved in 100 g of benzene . It raises boiling point by 1^(@)C then moles mass of the solute is ______.

(a) State Raoult's law for a solution containing volatile components. How does Raoult' s law become a special case of Henry's law? (b) 1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. Find the molar mass of the solute. (K_(f)" for benzene "=5.12 kg mol^(-1))

Knowledge Check

  • A solution containing 12.5 g of non-electrolyte substance in 185 g of water shows boiling point elevation of 0.80 K. Calculate the molar mass of the substance. ( K_b=0.52 K kg mol^(-1) )

    A
    `"53.06 g mol"^(-1)`
    B
    `"25.3 g mol"^(-1)`
    C
    `"16.08 g mol"^(-1)`
    D
    `"43.92 g mol"^(-1)`

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    When 0.9 g of a non-volatile solute was dissovled in 45 g of benezene, the elevation of boiling point is 0.88^@C . If K_b for benezene is 2.53 K kg "mol"^(-1) , Calculate the molar mass of solute.

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