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17 December, 19:03

A 0.468 g sample of pentane, C5H12, was burned in a bomb calorimeter. The temperature of the calorimeter and 1.00 kg of water in it rose from 20.45 °C to 23.65 °C. The heat capacity of the calorimeter by itself is 2.21 kJ/°C and the specific heat capacity of water is 4.184 J/g.°C What is the heat of combustion per mole of pentane?

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  1. 17 December, 20:01
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    E = 3,154.37 KJ

    The heat of combustion per mole of pentane is 3,154.37 KJ

    Explanation:

    Given;

    Change in temperature of system ∆T = 23.65-20.45 = 3.2 °C

    Mass of water m1 = 1 kg

    Specific heat capacity of water C1 = 4.184J/g°C = 4184J/kg °C

    Heat capacity of calorimeter mC2 = 2.21 kJ/°C = 2210J/°C

    Heat gained by both calorimeter and water is;

    H = (m1C1 + mC2) ∆T

    Substituting the values;

    H = (1*4184 + 2210) * 3.2

    H = 20460.8 J

    Mass of pentane burned = 0.468 g

    Molecular mass of pentane = 72.15g

    If 0.468g of pentane releases 20460.8 J of heat,

    72.15g of pentane will release;

    E = (72.15/0.468) * 20460.8 J

    E = 3154373.333333J

    E = 3,154.37 KJ

    The heat of combustion per mole of pentane is 3,154.37 KJ
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