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At 473 K, equilibrium constant K(c) for ...

At `473 K`, equilibrium constant `K_(c)` for decomposition of phosphorus pentachloride, `PCl_(5)` is `8.3 xx 10^(-3)` . If decomposition is depicted as,
`PCl_(5)(g) hArr Pcl_(3)(g) + Cl_(2) , Delta_(r)H^(ɵ) = 124.0 kJ "mol"^(-1)`
a) write an expression for `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 the effect on `K_(c)` if (i) more `PCl_(5)` is added (ii) pressure is increased (iii) the temperature is increased ?

Text Solution

Verified by Experts

`(a) K_(c) = [PCl_(3)][Cl_(2)]/[PCl_(5)]`
(b)`K' = 1/K_(c) = 1/(8.3 xx 10^(-3)) = 120.48`
(c ) (i) No effect as Kc is constant at constant temperature
(ii) No effect
(iii) As given reaction is endothermic, on increasing the temperature,`k_(f)` will increase.
As `K_(c) = k_(f)/k_(c)` ,Kc will increases with increases of temperature.
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At 473 K , equilibrium constant K_(c ) for decomposition of phosphorus pentachloride, PCl_(5) is 8.3xx10^(-3) . If decomposition is depicted as, PCl_(5)(g) hArr PCl_(3)(g)+Cl_(2)(g) Delta_(r)H^(Θ)=124.0 kJ mol^(-1) a. Write an expression for 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 the effect on K_(c ) if i. More PCl_(5) is added ii. Pressure is increased iii. The temperature is increased?

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