In a reaction: CO(g) + 2H₂(g) ⇌ CH₃OH(g) ∆H°= -92kJ/mol, if the concentrations of all species become constant, what will happen?
Correct answer: D. The equilibrium state will remain undisturbed
- A. The reaction will become faster
- B. The reaction will become slow
- C. The equilibrium state will be disturbed
- D. The equilibrium state will remain undisturbed
Explanation
When the concentrations of all reactants and products become constant, it signifies that the system has reached a state of dynamic equilibrium. The forward and reverse reaction rates are equal, and unless conditions change, the state will remain undisturbed.
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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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