For complete combustion of ethanol, `C_(2) H_(5) OH_((l)) + 3O_(2(g)) to 2CO_(2(g)) + 3H_(2) O_((l))`, the amount of heat produced as measured in bomb calorimeter is `1364.47 "kJ mol"^(-1)` at 25°C. Assuming ideality the Enthalpy of combustion, `Delta_(C) H`, for the reaction will be :
`(R= 8.314 "kJ mol"^(-1) )`

Options

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

Answer

C

Explanation

`C_(2) H_(5) OH_((l)) + 3O_(2(g)) to 2CO_(2(g)) + 3H_(2) O_((l))`
`Delta U = - 1364.47 "kJ mol"^(-1)`
`Deltan_(g) = -1`
`DeltaH = Delta U + Deltan_(g) RT`
`= -1364.47 - (1xx 8.314 xx 298)/( 1000)`
`=-1366.93 "kJ mol"^(-1)`