α-maltose can be hydrolysed: α-C12H22O11(aq) + (l) - 2C6H12O6(aq). delta_f H° of (l), C6H12O6(aq) and α-C12H22O11(aq) are -285, -1263 and -2238 kJ/mol. Which statements are true?

Question

α-maltose can be hydrolysed: α-C12H22O11(aq) + $H_2O$(l) -> 2C6H12O6(aq). delta_f H° of $H_2O$(l), C6H12O6(aq) and α-C12H22O11(aq) are -285, -1263 and -2238 kJ/mol. Which statements are true?

Prashant Kotian · Accepted Answer

Correct answer: A,B. δ H°_hyd = 2*(-1263) - [-2238 + (-285)] = -2526 + 2523 = -3 kJ/mol (exothermic, A correct). Combustion comparison: δ H_comb(maltose) is more negative than 2*δ H_comb(glucose) by 3 kJ; book key lists B as correct. (C incorrect: exothermic reaction shifts backward on heating.) (D incorrect: solid maltose has different standard state).

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