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25 November, 11:27

5.00 g of carbon were adiabatically burned to CO2 in a 2.00 kg copper calorimeter which contained 2.50 kg of water. The temperature increased by 14.1 °C.

Specific heats: copper, 0.385 J K⁻¹ g⁻¹; water, 4.184 J K⁻¹ g⁻¹.

a) Determine the heat of combustion of carbon ignoring any heat absorbed by the calorimeter.

b) Now determine the heat of combustion considering the heat absorbed by the calorimeter.

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  1. 25 November, 12:40
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    A. - 163.96kJ

    B. - 158.34kJ

    Explanation:

    Heat of combustion is the heat released when an element with oxygen at stp.

    Reaction for the combustion of carbon:

    C (s) + O2 (g) - -> CO2 (g)

    Enthalpy heat of combustion, C (using Hess law) = - 393.5 kJ/mol

    m = 5g

    Molecular weight = 12 g/mol

    No of moles = mass/molecular weight

    = 5/12

    = 0.417mol

    DH = - 393.5 * 0.417

    = - 163.96 kJ

    B. Heat absorbed by the calorimeter = heat evolve by combustion

    = mCH2ODT + mCcDT

    Where CH2O is the specific heat capacity of the water in the calorimeter

    Cc is the specific heat capacity of copper calorimeter

    = (2500*4.184*14.1) + (2000*0.385*14.1)

    = - 158343J

    = - 158.34kJ
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