Analysis of equilibrium reaction mixture @450 K in 1.00 L chamber for the reacti

Question

Analysis of equilibrium reaction mixture @450 K in 1.00 L chamber for the reaction:
CO (g) + H2O (g) <--> CO2 (g) + H2 (g)
showed [CO]=[H20]=0.230 M, [H2]=0.600M, and [CO2]=0.200M. To this equilibrium mixture 0.400 mol of carbon dioxide is added and equilibrium is allowed to reestablish.
a) what is the equilibrium constant for this reaction?
b) complete an ICE table
c) show that the equilibrium constant did not change because of the addition of the carbon dioxide to the original euilibrium mixture:

Explanation / Answer

a) K= [CO2][H2] / [CO][H2O] =0.2 x.6 / 0.23x .23=0.12/0.0529 = 2.26843

b) R CO H2O CO2 H2

I 0.43 .83 0 0

C -.2 .6 0.2 0.6

E .23 .23 0.2 0.6

C-

Le Chatelier's principle   

When a system at equilibrium is subjected to change in concentration, temperature, volume, or pressure, then the system readjusts itself to (partially) counteract the effect of the applied change and a new equilibrium is established.

so when we add CO to the mixture equlibirium sift to right

&so K(equ . constant ) is always constant.

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