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6 July, 20:15

The enthalpy of vaporization of liquid isopropyl alcohol is 45 kJ/mol. Calculate the energy required to vaporize 39.5 g of this compound.

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  1. 6 July, 20:39
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    29.625 kJ.

    Explanation:

    Enthalpy of vaporization, ∆Hvap which is also known as the latent heat of vaporization, is the amount of energy required to be added to a liquid substance to change the phase of a quantity of that substance into a gas.

    Molar mass of Isopropyl alcohol (C3H80) = (12*3) + (1*8) + 16

    = 60 g/mol.

    Number of moles = mass*molar mass

    = 39.5*60

    = 0.658 moles.

    Heat required = n * molar enthalpy of vapourisation.

    ∆Hvap = 45 kJ/mol.

    = 0.658*45

    = 29.625 kJ.
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