In the reaction; H2 + CO2 ⇌ H2O + CO. The decrease in the concentration of reactants and products cause the equilibrium to shift:
Correct answer: C. Nothing happens to the equilibrium
- A. Towards left
- B. Towards right
- C. Nothing happens to the equilibrium
- D. Equilibrium will shift towards both the directions
Explanation
At equilibrium, the system depends on the ratio of concentrations (the reaction quotient), not the absolute amounts. A proportional decrease in both reactants and products does not change the ratio, so the system remains at equilibrium. Thus, the equilibrium does not shift.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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