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Benzene burns in oxygen according to the following reactions.
$C_{6} H_{6} (l) + \frac{15}{2} O_{2} (g) \to 3 H_{2} O (l) + 6 C O_{2} (g)$
If the standard enthalpies of formation of $C_{6} H_{6} (l), H_{2} O (l) and C O_{2}$ are 11.7, $- 68.1$ and $- 94$ kcal/mole, respectively, the amount of heat that will liberate by burning 780 g of benzene is

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$7800 kcal$

$780 kcal$

$608.4 kcal$

$78 kcal$

answer is A.

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Detailed Solution

$Δ H combustion$ of Benzene $= \sum Δ_{f} H products - \sum Δ_{f} H reactants$

Enthalpy of combustion of one mole (78 g) of benzene is 780 kcal and for 780 g of benzene has 7800 kcal.

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