In a reaction: CO(g)+2H2(g)⇌CH3OH(g) ∆H°= -92kJ / mol, if concentration of hydrogen, carbon monoxide and methanol become constant at equilibrium, what will happen?
Correct answer: D. Equilibrium state will remain undisturbed
- A. Reaction will become faster
- B. Reaction will become slow
- C. Equilibrium state will be disturbed
- D. Equilibrium state will remain undisturbed
Explanation
Option d is correct because if the concentrations of all the reactants and products become constant at equilibrium, it means that the rates of the forward and reverse reactions have become equal. This indicates that the system is in a state of dynamic equilibrium, where the concentrations of all species remain constant over time.
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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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