posted by jon on .
Consider the following reactions and their equilibrium constants.
(NO(g) + 0.5Br2(g) <===> NOBr(g) Kp = 5.3
2NO(g) <===> N2(g) + O2(g) Kp = 2.1 x 1030
Use these equations and their equilibrium constants to determine the equilibrium constant for the following reaction:
N2(g) + O2(g) + Br2(g) <===> 2NOBr(g) Kp = ?
Write K expression for eqn 1.
(NOBr)/(NO)(Br2)^1/2 = 5.3.
Now square that.
(NOBr)^2/(NO)^2(Br2) = 5.3^2
Multiply that equation by Keq for equation #2 which is
(NOBr)^2/(N2)(O2) = 2.1 x 10^30
The (NO)^2 cancels and you are left with Keq for the reaction you want and K for the final reaction is just 5.3^2 x 2.1 x 10^30 = ??
Consider the following equilibrium:
2NO(g) N2(g) + O2(g); Keq = 2.1 × 1030