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24 March, 17:05

The temperature rises from 25.00°C to 29.00°C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ΔE rxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the calorimeter is 4.90 kJ/°C. The molar mass of sugar is 342.3 g/mol.

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  1. 24 March, 17:33
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    Answer: Hence the energy change is - 1918 kJ/mol

    Given:

    Initial temperature of calorimeter T1 = 25 C

    Final temperature T2 = 29 C

    Heat capacity of calorimeter c = 4.90 kJ/C

    Mass of sucrose (m) = 3.5 g

    Molar mass of sucrose (M) = 342.3 g/mol

    To determine:

    The energy change for the combustion of sucrose in kJ/mol

    Explanation:

    The change in temperature of calorimeter = T2 - T1 = 29 - 25 = 4 C

    Heat gained by the calorimeter when the temperature changes by 4 C is-

    = 4 C * 4.90 kJ / 1 C = 19. 6 kJ

    Now,

    Heat gained by calorimeter = heat lost during combustion of 3.5 g sucrose = - 19.6 kJ

    # moles of sucrose = 3.5 g/342.3 g. mole-1 = 0.01022 moles

    Energy change for the combustion reaction = - 19.6/0.01022 = - 1917.8 kJ/mol
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