Bromine monochloride, `(BrCl)` decomposes into bromine and chlorine and reaches the equilibrium.
`2BrCl_((g))hArrBr_(2(g))+Cl_(2(g))`
For which `K_(c)=32` at `500 K`. If initially pure `BrCl` is present at a concentration of `3.30xx10^(-3) mol litre^(-1)`, what is its molar concentration in the mixture at equilibrium?

Explanation

`{:(,2BrCl_((g)),hArr,Br_(2(g)),+,Cl_(2(g))),("Initial conc.",0.0033,,0,,0),("Conc. at equilibrium",(0.0033-a),,a//2,,a//2):}`
`K_(c)=([Br_(2)][Cl_(2)])/([BrCl]^(2))=32`
`:. ((a)/(2)xx(a)/(2))/((0.0033-a)^(2))=32`
or `(a)/(2xx(0.0033-a))=5.66`
`:. a=3xx10^(-3)`
`:. [BrCl]=3.3xx10^(-3)-3xx10^(-3)`
`=3xx10^(-4) mol litre^(-1)`