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How much quantity of ethylene glycol is added in 200 gm water to reduce the freezing point by 0.93K? Kf=1.86K. Kg `mol^(-1)`

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Ethylene glycol is used as antifreezing agent to prevent the freezing of water in car radiator in cold climate. Calculate the amount of ethylene glycol to be added to 5 kg of water to prevent it from freezing at -6^@C . Given K_f for water = 1.85 kg mol^-1 .

34.2 gm Sucrose (Molecular wt 342) is dissolved in 1000 gm of water. Find the freezing-point of the solution kf = 1.86 K Kg mol^-1

Knowledge Check

  • The temperature of a city was found tobe -9.30^@C . A car was used, whose radiator was filled with 5 L of water. What quantity of anti freezing agent ethylene glycol were added to water of radiator in order to use the car for travelling ? ( K_f of water 1.86 K kg mol^-1 )

    A
    3200 g
    B
    1670 g
    C
    1550 g
    D
    2100 g

  • KBr is 80% dissociated in aqueous solution. The freezing point of a 0.5 molal solution is K_f =1.86 K kg mol^-1

    A
    271.5 K
    B
    273 K
    C
    277 K
    D
    218 K

  • When 250 mg of eugenol is added to 100 g of camphor (k_f = 39.7 k molality^(-1)) , it lowered the freezing point by 0.62^@C . The molar mass of eugenol is :

    A
    `1.6 xx 10^2 g//mol`
    B
    `1.6 xx 10^4 g//mol`
    C
    `1.6 xx 10^3 g//mol`
    D
    200 g/mol

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    50g of antifreeze (ethylene glycol) is added to 200 g water. What amount of ice will separate out at -9.3^@C ?

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

    When 45 g of an unknown compound was dissolved in 500 g of water, the solution has freezing point of -0.93^(@)C (i) What is the molecular weight of compound ? (K_(f)=1.86) (ii) If empirical formula is CH_(2)O , what is the molecular formula of compound ?

    k_f for water is 1.86 k kg mol^(-1) If your automobile radiator holds 1.0 kg of water, how many grams of ethylene glycol (C_2H_6O_2) must you add to get the freezing point of the solution lowered to - 2. 8^@C ?

    A solution of 1.25 g of 'P' in 50g of water lowers freezing point by 0.3^@C . Molar mass of 'P' is 94. K_f(water) is 1.86 K kg mol^(-1). The degree of association of 'P' in water is [Assume dimerisation of P]

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