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19 May, 23:26

A certain chemical reaction releases 479 kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.36 J of heat energy to raise the temperature of this calorimeter by 1°C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 9.9°C.

a. How would you calculate the number of moles of reactant that were consumed?

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  1. 20 May, 02:28
    0
    6.94 x 10^-5 mol

    Explanation:

    It takes 3.36 J of heat energy to raise the temperature of this calorimeter by 1°C.

    The temperature of the calorimeter is found to rise by 9.9°C.

    So how much energy was required to achieve this?

    3.36 J = 1°C

    x = 9.9°C

    x = 9.9 * 3.36 / 1

    x = 33.264 J

    The chemical reaction releases 479 kJ of heat energy per mole of reactant consumed.

    So number of moles consumed is given as;

    479000 J = 1

    33.264 J = x

    x = 33.264 J * 1 / 479000J

    x = 6.94 x 10^-5 mol
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