$C_{2} H_{5} OH (l) + 3 O_{2} (g) ⟶ 2 {CO}_{2} (g) + 3 H_{2} O (g)$
During an experiment 10.00 g of ethanol is completely burned in air to release ${CO}_{2} (g)$ and $H_{2} O (g)$ as shown in the equation above. During the combustion, $296.6 kJ$ of heat energy is released. What is the molar enthalpy of combustion, $ΔH ° comb$

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$- 2966 kJ \times {mol}^{- 1}$

$- 1364 kJ \times {mol}^{- 1}$

$- 29.66 kJ \times {mol}^{- 1}$

$- 64.36 kJ \times {mol}^{- 1}$

answer is B.

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Detailed Solution

Molar enthalpy of combustion,

$- \frac{296.6}{10} \times 46 = - 1364.36$

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