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12 October, 00:07

A 1.00 g sample of nh4no3 is decomposed in a bomb calorimeter. the temperature increases by 6.12°c. what is the molar heat of decomposition for ammonium nitrate?

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  1. 12 October, 03:56
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    First, you have to know that this is an exothermic reaction as the heat increased as a product of the reaction.

    then, we need to get the heat change q = M*C*ΔT

    = 1 g * 1.23 KJ/C-1 * 6.12

    = 7.5 KJ

    and because of this is an exothermic reaction so,

    the heat of decomposition ΔH = - 7.5 KJ

    after that, we need to get the moles of NH4NO3:

    moles = mass / molar mass

    when the molar mass of NH4NO3 = 80.043 g/mol

    ∴ moles of NH4NO3 = 1g / 80.043 g/mol

    = 0.0125 moles

    So the decomposition then will be = ΔH / moles NH4NO3

    = - 7.5 KJ / 0.0125 moles

    = - 600 KJ. mol-1
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