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6 October, 06:24

How much energy is required to heat 87.1 g acetone (molar mass=58.08 g/mol) from a solid at - 154.0°C to a liquid at - 42.0°C? The following physical data may be useful. ΔHfus = 7.27 kJ/mol Cliq = 2.16 J/g°C Cgas = 1.29 J/g°C Csol = 1.65 J/g°C Tmelting = - 95.0°C.

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  1. 6 October, 06:39
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    The answer to the question above is

    The energy required to heat 87.1 g acetone from a solid at - 154.0°C to a liquid at - 42.0°C = 29.36 kJ

    Explanation:

    The given variables are

    ΔHfus = 7.27 kJ/mol

    Cliq = 2.16 J/g°C

    Cgas = 1.29 J/g°C

    Csol = 1.65 J/g°C

    Tmelting = - 95.0°C.

    Initial temperature = - 154.0°C

    Final temperature = - 42.0°C?

    Mass of acetone = 87.1 g

    Molar mass of acetone = 58.08 g/mol

    Solution

    Heat required to raise the temperature of solid acetone from - 154 °C to - 95 °C or 59 °C is given by

    H = mCsolT = 87.1 g * 1.65 J/g°C * 59 °C = 8479.185 J

    Heat required to melt the acetone at - 95 °C = ΔHfus*number of moles =

    But number of moles = mass: (molar mass) = 87.1:58.08 = 1.5

    Heat required to melt the acetone at - 95 °C = 1.5 moles*7.27 kJ/mol = 10.905 kJ

    The heat required to raise the temperature to - 42 degrees is

    H = m*Cliq*T = 87.1 g * 2.16 J/g°C * 53 °C = 9971.21 J

    Total heat = 9971.21 J + 10.905 kJ + 8479.185 J = 29355.393 J = 29.36 kJ

    The energy required to heat 87.1 g acetone from a solid at - 154.0°C to a liquid at - 42.0°C is 29.36 kJ
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