Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074



Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The value of ΔU for the decomposition of 7.647 g of ammonium nitrate can be measured in a bomb calorimeter. The reaction that occurs is

NH4NO3(s) → N2O(g) + 2 H2O(g)

The temperature of the calorimeter, which contains 415 g of water, increases from 18.90 °C to 20.72 °C. The heat capacity of the bomb is 155 J/K. What is the value of ΔU for this reaction, in kl/mol?


Interpretation Introduction


The change in internal energy has to be calculated.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.


Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity, ΔT= change in temperature.


Given ΔT=1.82K

Specific heat capacity of water is 4.184J/gK

Heat capacity of calorimeter is 155J/K

Mass of the water is 415g

Using specific capacity of heat equation

  q=C×m×ΔT, the values calculated.

Heat absorbed by the calorimeter =155J/K×1.82K =282J

Heat absorbed by water = 415g×4.184J/gK×1.82K = 3160J

Total heat absorbed =282J+3160J

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