A quantity of 1.6 g sample of is decomposed in a bomb calorimeter. The temperature of the calorimeter decreases by 6.0 K. The heat capacity of the calorimeter system is 1.25 kJ/K. The molar heat of de

Question

A quantity of 1.6 g sample of $NH_4NO_3$ is decomposed in a bomb calorimeter. The temperature of the calorimeter decreases by 6.0 K. The heat capacity of the calorimeter system is 1.25 kJ/K. The molar heat of decomposition for $NH_4NO_3$ is

Prashant Kotian · Accepted Answer

Correct answer: D. Heat absorbed by the calorimeter during the decomposition process: q_cal = C * δ T = 1.25 kJ/K * (-6.0 K) = -7.5 kJ. Since the calorimeter temperature decreases, the reaction is endothermic, absorbing heat from the surroundings. Thus, q_rxn = +7.5 kJ. Moles of decomposed: n = mass / molar mass = 1.6 g / 80.0 g/mol = 0.02 mol. Molar heat of decomposition: δ H = q_rxn / n = +7.5 kJ / 0.02 mol = +375 kJ/mol.

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