in this figure it\'s showing how they can substitute the number of molecules of

Question

in this figure it's showing how they can substitute the number of molecules of each reactant or product into the equilibrium-constant expression. My question is how did they figure out the molecules of each reactant or product when there was no number given. The only number that was given was Keq equals 16. So how did they get 81?

Keu-16 picture in Figure 12.17 shows a mixture of these rea volume. The equilibrium constant expression for thi ICOJ[H,O] eq f this system is at equilibrium, we can substitute the reactant or product into the equilibrium constant ex

Explanation / Answer

The given equilibrium reaction is,

CO (g) + H2O (g) <====> CO2 (g) + H2 (g) Kc = 16

While looking at the direction in whic the equilbrium would shift, we compare the reaction quotient with the equilbrium constant.

The image must have been showing the Q value at certain concentrations.

Q = [CO2] [ H2]/ [CO][H2O]

When the reaction is 90 % complete, the following concentrations would be observed. Assume, we start with 10 mol/L each of CO and H2O.

Q =  [CO2] [ H2]/ [CO][H2O] =  [9] [9]/ [1][1] =81

Here Q = 81 and Kc = 16

Q > Kc

So, the equilibrium would shift towards left to compensate for the extra amount of products formed. (Products react aback to form reactants)

CO (g) H2O (g) CO2 (g) H2 (g) Initial 10 10 0 0 Change -9 -9 +9 +9 Equilibrium 1 1 9 9

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