Ans :-
Combustion reaction of C2H6 is :
2C2H6 (g) + 7O2 (g) ----------------> 4CO2 (g) + 6H2O (l)
Because,
ΔH0rxn = [Sum of enthalpy of formation of products] - [Sum of enthalpy of formation of reactants]
= [4 x ΔHf0 of CO2 (g) + 6 x ΔHf0 of H2O (l) ] - [ 2 x ΔHf0 of C2H6 (g) + 7 x ΔHf0 of O2 (g)]
= [ 4 x (–393.5 KJ/mol) + 6 x (–285.8 KJ/mol)] - [ 2 x (–84.0 KJ/mol) + 7 x 0.0 KJ/mol]
= [ - 1574 KJ- 1714.8 KJ] - [ - 168 KJ]
= - 3288.8 KJ+ 168 KJ
= - 3120.8 KJ
So, enthalpy of combustion for 2 moles of C2H6 (g) = - 3120.8 KJ
and
Enthalpy of combustion for 1 moles of C2H6 (g) = - 3120.8 KJ / 2 mol = -1560.4 KJ/mol
Therefore, Enthalpy of combustion of C2H6 (g) = ΔH0rxn = - 1560.4 KJ/mol ethane |
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on 25 of 25 > What is the heat of combustion of ethane, C,H, in kilojoules per mole of ethane? Enthalpies of formation can be found in the table of thermodynamic properties. AH = kJ/mol ethane
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