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For complete combustion of ethanol, $C_{2} H_{5} OH (l) + 3 O_{2} (g) ⟶ {CO}_{2} (g) + 3 H_{2} O (l)$ , the heat produced as measured in bomb calorimeter, is $1364.47 kJ {mol}^{- 1}$ at 25°C. Assuming ideality the enthlapy of combustion, $Δ_{c} H,$ for the reaction will be $(R = 8.314 {JK}^{- 1} {mol}^{- 1})$

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detailed solution

Correct option is B

For the given reaction, $Δ v_{g} = - 1$ . Hence

$\begin{array}{l} Δ H^{\circ} = Δ U^{\circ} + (Δ v_{g}) R T = (- 1364.47 kJ {mol}^{- 1}) + (- 1) (8.314 \times 10^{- 3} {kJK}^{- 1} {mol}^{- 1}) (298 K) \\ = - 1366.95 kJ {mol}^{- 1} \end{array}$

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For complete combustion of ethanol, C2H5OH(l)+3O2(g)⟶CO2(g)+3H2O(l), the heat produced as measured in bomb calorimeter, is 1364.47kJmol−1 at 25°C. Assuming ideality the enthlapy of combustion, ΔcH, for the reaction will be R=8.314JK−1mol−1