For complete combustion of ethanol, $C_{2} H_{5} OH (l) + 3 O_{2} (g) ⟶ 2 {CO}_{2} (g) + 3 H_{2} O (l)$ the amount of heat produced as measured in bomb calorimeter, is $1364 .47 kJ {mol}^{- 1} at 25^{\circ} C$ Assuming ideality the enthalpy of combustion, $Δ_{c} H$ for the reaction will be: $(R = 8 .314 kJ {mol}^{- 1})$

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$- 1361 .95 kJ {mol}^{- 1}$

$- 1460 .95 kJ {mol}^{- 1}$

$- 1350 .50 kJ {mol}^{- 1}$

-1366.95 kJ moI^-1

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Detailed Solution

$C_{2} H_{5} OH (ℓ) + 3 O_{2} (g) ⟶ 2 {CO}_{2} (g) + 3 H_{2} O (ℓ)$
Bomb calorimeter gives $∆$ U f the reaction
Given, $ΔU = - 1364 .47 kJ {mol}^{- 1}$
${Δn}_{g} = - 1$
$ΔH = ΔU + {Δn}_{g} RT = - 1364.47 - \frac{1 \times 8.314 \times 298}{1000} = - 1366.93 kJ {mol}^{- 1}$