At 473K, equilibrium constant `K_(C)` for the decompositioni of phosphorus pentachloride, `PCl_(5)` is `8.3xx10^(-3)`. If the decomposition is depicted as:
`PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g)DeltaH=124.0 kJ "mol"^(-1)`
a. Write an expression of `K_(c)` for the reaction.
b. What is the value of `K_(c)` for the reverse reaction at the same temperature?
c. What would be effect on `K_(c)` if
(i) more `PCl_(5)` is added (ii) pressure is increased (iii) the temperature in increased.

Explanation

Given
`PCl_(5(g)) hArr PCl_(3(g))+Cl_(2(g)) DeltaH=124.0` kJ/mol
`K_(C)=8.3xx10^(-3)`
`K_(c)=([PCl_(3)][Cl_(2)])/([PCl_(5)])`