[latex]\Delta H_0[/latex] (enthalpy of combustion at reference temperature [latex]T_o[/latex]) for benzene vapour ([latex]C_6 H_6[/latex]) at 25°C is – 3301000 kJ/mole with the [latex]H _2 O[/latex] in the liquid phase. Calculate [latex]\Delta H_0[/latex] for the [latex]H _2 O[/latex] in the vapour phase.

If [latex]H _2 O[/latex] remains as a vapour the heat transferred to the surroundings will be less than when the vapour condenses by the amount due to the change in enthalpy of the vapour during condensation at the reference temperature. [latex]\Delta H_0 \text { (vapour) }=\Delta H_0 \text { (liquid) }+m_s h_{\text {fgo }}[/latex] where, [latex]m_s=[/latex] Mass of [latex]H _2 O[/latex] formed, and [latex]h_{f g o}=[/latex] Change in enthalpy of steam between saturated liquid and saturated vapour at the reference temperature [latex]T_o[/latex] = 2441.8 kJ at 25°C For the reaction : [latex]C _6 H _6+7.5 O _2 \longrightarrow 6 CO _2+3 H _2 O[/latex] 3 moles of [latex]H _2 O[/latex] are formed on combustion of 1 mole of [latex]C_6 H_6[/latex] ; 3 moles of [latex]H _2 O[/latex] = 3 × 18 = 54 kg [latex]H _2 O[/latex] ∴ [latex]\Delta H _0(\text { vapour })=-3301000+54 \times 2441.8=- 3 1 6 9 1 4 3[/latex] kJ/mole.

Question 11.31: ΔH0 (enthalpy of combustion at reference temperature T0) for...

Engineering Thermodynamics

$\Delta H_0$ (enthalpy of combustion at reference temperature $T_o$ ) for benzene vapour ( $C_6 H_6$ ) at 25°C is – 3301000 kJ/mole with the $H _2 O$ in the liquid phase. Calculate $\Delta H_0$ for the $H _2 O$ in the vapour phase.

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