Calculate the value of equilibrium constant for the reaction:
`A_((g))+B_((g))hArrC_((g))+D_((g))+E_((g))` at `300 K` and constant pressure. All the reactants and products obey ideal gas nature. Given `DeltaU^(@)=-90.0 kcal`, `DeltaS^(@)=100 calK^(-1)`.

Explanation

For `A_((g))+B_((g))hArrC_((g))+D_((g))+E_((g))`
`Deltan=1 :. DeltaH^(@)=DeltaU^(@)+DeltanRT`
`=-90xx10^(3)+1xx300xx2=-89400cal`
Now `DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
`=-89400-300xx100=-119400cal`
Now `-DeltaG^(@)=2.303RT log K_(p)`
`119400=2.303xx2xx300 log K_(p)`
`:. K_(p)=2.56xx10^(86)`