One mole of C_2H_5OH_{(l)} was completely bur | vedclass

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(A) The balanced chemical equation for the combustion of ethanol is: $C_2H_5OH_{(l)} + 3O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$ The standard en

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$2y + 3z - x$

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(A) The balanced chemical equation for the combustion of ethanol is: $C_2H_5OH_{(l)} + 3O_{2(g)} ightarrow 2CO_{2(g)} + 3H_2O_{(l)}$ The standard enthalpy of reaction $\Delta_rH^{\ominus}$ is calculated using the formula: $\Delta_rH^{\ominus} = \sum \Delta_fH^{\ominus}(	ext{products}) - \sum \Delta_fH^{\ominus}(	ext{reactants})$ Substituting the given values: $\Delta_rH^{\ominus} = [2 	imes \Delta_fH^{\ominus}(CO_{2(g)}) + 3 	imes \Delta_fH^{\ominus}(H_2O_{(l)})] - [\Delta_fH^{\ominus}(C_2H_5OH_{(l)}) + 3 	imes \Delta_fH^{\ominus}(O_{2(g)})]$ Since $\Delta_fH^{\ominus}$ for an element in its standard state $(O_{2(g)})$ is $0$: $\Delta_rH^{\ominus} = [2y + 3z] - [x + 3(0)] = 2y + 3z - x \ kJ \ mol^{-1}$

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