Question #0799c
1 Answer
#bb(P_(BrCl) = "0.222 bar")#
As a note, I assume by "final" you mean after the vessel pumping was stopped. If the equilibrium partial pressure of
#P_i^2/(0.345) = 0.0172#
But if that were the case,
We don't know the reaction, but it doesn't matter. We know that the number of bromine and chlorine atoms are
Furthermore,
#2"BrCl"(g) rightleftharpoons "Br"_2(g) + "Cl"_2(g)#
Therefore:
#K_P = P_i^2/(0.345 - 2P_i) = 0.0172# where
#P_i# is the partial pressure of either the bromine or chlorine product, and#"0.345 bar"# is the NON-EQUILIBRIUM partial pressure of#"BrCl"# .
A nice trick @anor277 loves to use is a recursive small
#P_i ~~ sqrt(K_Pcdot"0.345 bar") ~~ "0.0770 bar"#
As it is, the approximation fails badly, because
#P_i/P_(BrCl) xx 100% = "0.0770 bar"/"0.345 bar" xx 100% > 5%# ...
But, if we take the converged
#P_i^"*" = sqrt(K_P("0.345 bar" - 2P_i))# ,
we get:
#P_i^"*" -> -> "0.0617 bar"#
And to check:
#0.0172 stackrel(?" ")(=) (0.0617^2)/(0.345 - 2*0.0617) = 0.0172#
So, the equilibrium partial pressure of
#color(blue)(P_(BrCl)) = "0.345 bar" - 2*"0.0617 bar" = color(blue)("0.222 bar")#
I assume you can determine the equilibrium partial pressures of