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3 January, 10:22

A quantity of 1.922 g of methanol (CH3OH) was burned in a constant-volume bomb calorimeter. Consequently, the temperature rose by 5.72°C. If the heat capacity of the bomb plus water was 9.47 kJ / °C, calculate the molar heat of combustion of methanol.

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  1. 3 January, 12:55
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    872.28 kJ/mol

    Explanation:

    The heat released is:

    ΔH = C*ΔT

    where ΔH is the heat of combustion, C is the heat capacity of the bomb plus water, and ΔT is the rise of temperature. Replacing with dа ta:

    ΔH = 9.47*5.72 = 54.1684kJ

    A quantity of 1.922 g of methanol in moles are:

    moles = mass / molar mass

    moles = 1.992/32.04 = 0.0621 mol

    Then the molar heat of combustion of methanol is:

    ΔH/moles = 54.1684/0.0621 = 872.28 kJ/mol
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