(D) The molar mass of $NH_4NO_3$ is $80 \ g/mol$.Heat evolved $(q)$ is calculated as $q = C \times \Delta T = 1.23 \ kJ/K \times 6.12 \ K = 7.5276 \ k

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(D) The molar mass of $NH_4NO_3$ is $80 \ g/mol$.Heat evolved $(q)$ is calculated as $q = C \times \Delta T = 1.23 \ kJ/K \times 6.12 \ K = 7.5276 \ kJ$.This heat is released by $1 \ g$ of $NH_4NO_3$.The molar heat of decomposition is calculated as $\Delta H = q \times \text{Molar Mass} = 7.5276 \ kJ/g \times 80 \ g/mol = 602.2 \ kJ/mol$.Since the decomposition is an exothermic process occurring in a bomb calorimeter,the value is negative: $-602 \ kJ/mol$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

One gram sample of $NH_4NO_3$ is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by $6.12 \ K$. The heat capacity of the system is $1.23 \ kJ/K$. What is the molar heat of decomposition for $NH_4NO_3$ in $kJ/mol$?

AIIMS 2003 All AIIMS

A
$-7.53$
B
$-398.1$
C
$-16.1$
D
$-602$

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One gram sample of $NH_4NO_3$ is decomposed in a bomb calorimeter. The temperature of the calorimeter increases by $6.12 \ K$. The heat capacity of the system is $1.23 \ kJ/K$. What is the molar heat of decomposition for $NH_4NO_3$ in $kJ/mol$?

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Which of the following is (are) an endothermic reaction?

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Enthalpy of fusion and enthalpy of vaporization for water respectively are $6.01 \ kJ \ mol^{-1}$ and $45.07 \ kJ \ mol^{-1}$ at $0^{\circ}C$. What is enthalpy of sublimation at $0^{\circ}C$?

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