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Enthalpy of combustion of ${CH}_{4}, C_{2} H_{6} and C_{3} H_{8} are - 210, - 370 and - 530 kcal / mol$ respectively. The approximate value of enthalpy of combustion of n-hexane is

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$- 1170 \frac{kcal}{mol}$

$- 590 \frac{kcal}{mol}$

$- 1010 \frac{kcal}{mol}$

$- 750 \frac{kcal}{mol}$

answer is C.

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Detailed Solution

For each $- {CH}_{2}$ the enthalpy of combustion is increased by 160 kcal/mol.

$∴ ∆_{comb} H (C_{6} H_{6}) = - 210 - 5 \times 160 = - 1010 \frac{kcal}{mol}$

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