Question

Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration...

Consider the following system at equilibrium CH4(g) + 2H2O(g) ↔ CO2(g) + 4H2(g). Suppose the concentration of H2O is increased.

(a) In which direction does the reaction shift to reestablish equilibrium?

(b) What happens to the concentrations of CH4, CO2, and H2 as the reaction shifts to reestablish equilibrium?

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Answer #1

Hi, to be simple when you increase concentration on either side of the reaction, the reaction shifts to the other side to decrease the increased concentration. Since the concentration of H2O is increased, the system will shift towards the product side to produce more CO2 and H2 so that the concentration on the reactant side can be minimized until the reaction is reestablished.

So, in this case the equilibrium will shift to right since you have increased concentration on the left side.

Since, the reaction has turned to right hand direction to restore equiblium, the concentration on right hand side will increase will it will decrease on left hand side. The concentration of CH4 will decrease will H2O and the concentration of CO2 and H2 will increase.

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