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

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:

Answered by Abhisek | 1 year ago

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