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)

Asked by Pragya Singh | 1 year ago |  80

##### 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:

Answered by Abhisek | 1 year ago

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