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InterviewSolution
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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? |
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Answer» `{:(,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)` |
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