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

Answer

C

Explanation

In bomb calorimeter `DeltaU=-1364.47kJ" "mol^(-1)` lt brgt we know,
`DeltaH=DeltaU+Deltan_(g)RT` . . (i)
`Deltan_(g)=2-3=-1`
From eq n. (i) `DeltaH=-1364.47xx10^(3)+(-1)xx3.314xx298`
`=-1364470-2477.572` lt brgt `=-1366947.572J " " mol^(-1)`
`=-1366.95kJ" "mol^(-1)`