Heat evolved in the complete combustion of 1.026 kg sucrose at constant pressure will be<br> — Thermodynamics and Thermochemistry Chemistry Question
Question
Heat evolved in the complete combustion of 1.026 kg sucrose at constant pressure will be<br>$\text{C}_{12}\text{H}_{22}\text{O}_{11}\text{(s)} + 12\text{O}_2\text{(g)} \to 12\text{CO}_2\text{(g)} + 11\text{H}_2\text{O(l)}; \Delta H = -5.65 \times 10^3\text{ kJ}$
Answer: A
💡 Solution & Explanation
Molar mass of sucrose is $342\text{ g/mol}$. Mass is $1.026\text{ kg} = 1026\text{ g}$. Moles = $1026 / 342 = 3.0\text{ moles}$. Total heat evolved = $3 \times 5.65 \times 10^3\text{ kJ} = 16.95 \times 10^3\text{ kJ} = 1.695 \times 10^4\text{ kJ}$.
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