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Ethylene glycol in water is commonly use...

Ethylene glycol in water is commonly used as an antifreeze solution is car radiators. 12.4 g of this substance is dissolved in 100 g of water (`k_(f)` and `k_(b)` for water are `1.86 k m^(-1)` and `0.52 k m^(-1)` respectively).
What is the mole fraction of ethylene glycol in the solution ?

Text Solution

AI Generated Solution

To find the mole fraction of ethylene glycol in the solution, we will follow these steps: ### Step 1: Calculate the number of moles of ethylene glycol. The formula to calculate the number of moles is: \[ \text{Number of moles} = \frac{\text{Given mass}}{\text{Molar mass}} \] For ethylene glycol (C₂H₆O₂), the molar mass is calculated as follows: ...
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Ethylene glycol ("molar mass"=62 g mol^(-1)) is a common automobile antyfreeze. Calculate the freezing point of a solution containing 12.4 g of this substance in 100 g of water. (Given K_(f) for water = 1.86 K kg mol^(-1))

Calculate the freezing point depression and boiling point elevation of a solution of 10.0 g of urea (M_(B)=60) in 50.0 g of water at 1 atm . pressure. K_(b) and K_(f) for water 0.52^(@)C m^(-1) and 1.86^(@)C m^(-1) respectively.

Knowledge Check

  • A solution of ‘X’ (molar mass 60 g mol^(-1) ) in water boils at 100.18^@C at the atmospheric pressure.If K_f and K_b for water are 1.86 and 0.52 K kg mol^(-1) respectively, then the freezing point of the solution is :

    A
    `-65.4^@C`
    B
    `-0.654^@C`
    C
    `65.4^@C`
    D
    `+0.654^@C`

  • A solution containing 10 mole of ethylene glycol dissolved in 1000 g of water ( K_(f) = 1.86 K "molality^(-1) will freeze at:

    A
    273 K
    B
    2.544 K
    C
    254.4 K
    D
    25.44 K

  • When 40 g of substance is dissolved in 1000 g g of water, its freezing point is depressed by 1.86^@C. K_f for water is 1.86^@C mol^-1 then find the molar mass of the solute.

    A
    4
    B
    10
    C
    40
    D
    400

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    Calculate the amount of ice that will separate out on cooling containing 50 g of ethylene glycol in 200 g of water to -9.3^(@)C (K_(f) for water = 1.86 K mol^(-1) kg )

    Calculate the amount of ice that will separate out on cooling a solution containing 50g of ethylene glycol in 200g water to -9.3^(@)C ( K_(f) for water = 1.86 "K kg mol"^(-1) )

    What is the g-molecular mass of nonionizing solid if 10 g of this solid dissolved in 100 g of water, forms a solution which froze at -1.22^(@) C ? (K_(f)=1.86 K kg mol^(-1))

    Ethylene glycol is used as an antifreeze in a cold climate. Mass of ethylene glycol which should be added to 4 kg of water to prevent it from freezing at -6^(@)C will be (K_(f) for water = 1.86 Kkg mol^(-1) , and molar mass of ethylene glycol =62 g mol^(-1))

    Ethylene glycol is used as antifreeze in a cold climete. Mass of ethylene glycol which should be added to 4 kg of water = 1.86 K kg mol^(-1) , molar mass of ethylene glycol = 62 g mol,^(-1) )

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