`DeltaH^(Theta)` and `DeltaS^(Theta)` for the reaction:
`Br_(2)(l) +CI_(2)(g) hArr 2BrCI(g)`
at `298K` are `29.3 kJ mol^(-1)` and `104.1 J K^(-1) mol^(-1)`, respectively. Calculate the equilibrium constant for the reaction.

Explanation

`DeltaG^(Theta) =DeltaH^(Theta) -T DeltaS^(Theta)`
`= 29.3 xx 10^(3) - 298 xx 104.1 =- 1721.8 J mol^(-1)`
`log K =- (DeltaG^(@))/(2.303 RT) =- (-1721.8)/(2.303xx8.314xx298) = 0.3018`
`K = 2.003`