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

A
$- 1350.50 kJ {mol}^{- 1}$
B
$- 1366.95 kJ {mol}^{- 1}$
C
$- 1361.95 kJ {mol}^{- 1}$
D
$- 1460.50 kJ {mol}^{- 1}$

Solution:

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

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

Solution:

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