Answer:
Given balanced combustion reaction,
2 H3COH (g) + 3 O2 (g) 2 CO2 (g) + 4 H2O (g)
By knowing Standard enthalpies of formation of each reactant and product, the standard enthalpy of the reaction is given as,
ΔH°rxn = Σ ΔH°f (products) − Σ ΔH°f (reactants).
For above combustion reaction,
ΔH°rxn = [4*ΔH°f H2O(g) + 2* ΔH°f CO2 (g)] - [2*ΔH°f CH3OH(g) + 3* ΔH°f O2 (g)]
By placing standard enthalpies of formation of H3COH (g), O2 (g), CO2 (g), H2O (g) from literature we have,
ΔH°rxn = [4*(−241.818 kJ/mol) + 2*(−393.509 kJ/mol)] - [2*(−201.0 kJ/mol) + 3*(0 kJ/mol)]
ΔH°rxn = - 1352.290 kJ/mol
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