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. `-1366.95kJ"mol"^(-1)`
B. `-1361.95kJ"mol"^(-1)`
C. `-1460.95kJ"mol"^(-1)`
D. `-1350.50kJ"mol"^(-1)`

Answer

A

Explanation

`C_(2)H_(5)OH(1)+3O_(2)(g)to2CO_(2)(g)+3H_(2)O(1)`
Bomb callorimeter gives `Delta U` of the reaction,
Given `DeltaU=-1364.47kJ"mol"^(-1)`
`Delta_(g)=1`
`DeltaH=DeltaU+Deltan_(g)RT=-1364.47-(1xx8.314xx298)/1000`
`=-1366.95kJ"mol"^(-1)`