For the complete combustion of ethanol, `C_(2)H_(5)OH(l)+3O_(2)(g)rarr2CO_(2)(g)+3H_(2)O(l)` the amount of heat produced as measured in bomb calorimeter is `1364.47KJ mol^(-1)` at `25^(@)C` . Assuming ideality, the enthalpy of combustion, `DeltaH_(C)` , for the reaction will be
`[R=8.314JK^(-1)mol^(-1)]`

Options

A. `-1366.95 kJ mol^(-1)`
B. `-1361.95 kJ mol^(-1)`
C. `-1460.50 kJ mol^(-1)`
D. `-1350.50 kJ mol^(-1)`

Answer

A

Explanation

Amount of heat produced in bomb calorimeter,
`DeltaU=-1364.47 kJ mol^(-1)`
Enthalpy of a combustion reaction is
`DeltaH=DeltaU+Deltan_(g)RT`
`Deltan_(g)=2-3=-1`
`DeltaH=-1364.47-2.477`
Thus,
`=-1366.947 kJ mol^(-1)`
Hence, the enthalpy of combustion, `Delta_(C) H` for the given reaction will be `-1366.47 kJ mol^(-1)`