Calculate `DeltaH^(@)` for the reaction between ethene and water to form ethyl alcohol from the following data:
`Delta_(c)H^(@)C_(2)H_(5)OH_((1))=-136kJ`
`Delta_(c)H^(@)C_(2)H_(4(g))=-1410kJ`
Does the calculated `DeltaH^(@)` represent the enthalpy of formation of liquid ethanol ?

Explanation

`CH_(2)=CH_(2(g))+H_(2)O_((g))hArrCH_(3)CH_(2)OH_((g))`
`DeltaH=sumnH^(@)f_("products")-sumnH^(@)f_("reactants")`
`=(1xx-1368)-[(1xx(-1410)+(1xx-286))`
`=-1368-[-1410-286]`
`=-168-[-1696]`
`DeltaH=328J//mol`
No calculated value does not represent the enthalpy of formation of liquid enthanol. Standard enthalpy of formation for liquid ethanol is `-277.6kJ//mol.`