For a reversible reaction, if the concentrations of the reactants are doubled, at constant temperature the reaction will
Correct answer: D. move towards right
- A. stand still
- B. slow down
- C. speed up in reverse direction
- D. move towards right
Explanation
If the concentrations of the reactants are increased in a reversible reaction, the reaction will shift towards the side with fewer moles of gas, or the side with a higher value of Kc, which usually means that the reaction will move towards forming more products. This is known as Le Chatelier's principle, which states that a system at equilibrium will respond to a change in conditions by shifting its equilibrium position in a way that tends to counteract the change. If the concentrations of the reactants are increased, the equilibrium will shift towards the products to counteract the increase in reactants. This is assuming that the temperature is constant.
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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.
Practise Chemical Equilibrium
625 free Chemical Equilibrium MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
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