A sample of pure PCl5 was introduced into an evacuated vessel at 473 K. After equilibrium was attained, the concentration of PCl5 was found to be \( 0.5\times 10^{-1}\). If value of Kc is \( 8.3\times 10^{-3}\), what are the concentrations of PCl3 and Cl2 at equilibrium?
PCl5(g) ⇌ PCl3(g) + Cl2(g)
1 Answer
Solution :-
Consider the conc. Of both PCl3 and Cl2 at equilibrium be x molL–1. The given reaction is:
PCl5(g) ⇌ PCl3(g) + Cl2(g)
At equilibrium \( 0.5\times 10^{-10}molL^{-1}\) , x mol L-1 , x mol L-1
It is given that the value of equilibrium constant ,
Kc is \( 8.3\times 10^{-10}molL^{-3}\)
Now we can write the expression for equilibrium as:
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