The heat capacity of bomb calorimeter is 500 J/°C. A 2°C rise in temperature has been observed on th — Thermodynamics and Thermochemistry Chemistry Question

💡 Solution & Explanation

The heat absorbed by the bomb calorimeter (constant-volume heat, δ E) is: q_cal = C * δ T = 500 J/°C * 2°C = 1000 J = 1 kJ. Since this is an exothermic combustion reaction, the heat of reaction is q_rxn = -1 kJ for 0.1 g of $CH_4$. Moles of $CH_4$ (molar mass = 16 g/mol) = 0.1 g / 16 g/mol = 1/160 mol. The internal energy change δ E per mole of methane is: δ E = q_rxn / n = -1 kJ / (1/160 mol) = -160 kJ/mol.