Heat evolved in the complete combustion of 1.026 kg sucrose at constant pressure will be: C12H22O11(s) + 12(g) - 12(g) + 11(l); δ H = -5.65 × 10^3 kJ

Question

Heat evolved in the complete combustion of 1.026 kg sucrose at constant pressure will be: C12H22O11(s) + 12$O_2$(g) -> 12$CO_2$(g) + 11$H_2O$(l); δ H = -5.65 × 10^3 kJ

Prashant Kotian · Accepted Answer

Correct answer: A. Molar mass of sucrose (C12H22O11) = 342 g/mol. Moles of sucrose in 1.026 kg (1026 g): n = 1026 g / 342 g/mol = 3.0 mol. Since combustion of 1 mole releases 5.65 * 10^3 kJ, the heat evolved for 3 moles is: q = 3.0 * 5.65 * 10^3 kJ = 1.695 * 10^4 kJ.

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