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19 April, 16:08

A quantity of 1.922 g of methanol (ch3oh) was burned in a constant-volume bomb calorimeter. consequently, the temperature rose by 5.14°c. if the heat capacity of the bomb plus water was 8.69 kj / °c, calculate the molar heat of combustion of methanol.

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  1. 19 April, 16:35
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    The formula for calculating the amount of energy or heat released is:

    ΔH = C ΔT

    where ΔH is heat of combustion, C is heat capacity, while ΔT is change in temperature

    ΔH = 8.69 kJ / °C * (5.14°C)

    ΔH = 44.67 kJ

    Then we calculate the moles of CH3OH which has molar mass of 32.04 g/mol:

    moles = 1.922 / 32.04 = 0.05999 mol

    SO the molar heat of combustion is:

    ΔHm = 44.67 kJ / 0.0599875 mol

    ΔHm = 744.60 kJ / mol
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