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20 April, 13:28

When 1.98g of a hydrocarbon is burned in a bomb calorimeter, the temperature increases by 2.06∘C. If the heat capacity of the calorimeter is 69.6 J∘C and it is submerged in 944mL of water, how much heat (in kJ) was produced by the hydrocarbon combustion?

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  1. 20 April, 13:38
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    8.3 kJ

    Explanation:

    In this problem we have to consider that both water and the calorimeter absorb the heat of combustion, so we will calculate them:

    q for water:

    q H₂O = m x c x ΔT where m: mass of water = 944 mL x 1 g/mL = 944 g

    c: specific heat of water = 4.186 J/gºC

    ΔT : change in temperature = 2.06 ºC

    so solving for q:

    q H₂O = 944 g x 4.186 J/gºC x 2.06 ºC = 8,140 J

    For calorimeter

    q calorimeter = C x ΔT where C: heat capacity of calorimeter = 69.6 ºC

    ΔT : change in temperature = 2.06 ºC

    q calorimeter = 69.60J x 2.06 ºC = 143.4 J

    Total heat released = 8,140 J + 143.4 J = 8,2836 J

    Converting into kilojoules by dividing by 1000 we will have answered the question:

    8,2836 J x 1 kJ/J = 8.3 kJ
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