A quantity of 0.3 g of carbon was converted into producing 2400 cal of heat. When 0.6 g of carbon wa — Thermodynamics and Thermochemistry Chemistry Question

💡 Solution & Explanation

Heat of formation of $\text{CO}_2$: 0.3 g C (0.025 mol) releases 2400 cal $\implies \Delta H_f(\text{CO}_2) = -96\text{ kcal/mol}$. Heat of formation of CO: 0.6 g C (0.05 mol) releases 1400 cal $\implies \Delta H_f(\text{CO}) = -28\text{ kcal/mol}$. For $\text{CO} \to \text{CO}_2$, $\Delta H = -96 - (-28) = -68\text{ kcal/mol}$. 0.7 g CO = 0.025 mol. Heat produced = $0.025 \times 68000\text{ cal} = 1700\text{ cal}$.