A chemical reaction has reached to a state of dynamic equilibrium at certain temperature.Which of the following statements is incorrect?
Correct answer: D. The reaction has stopped completely
- A. Concentration of the reactants remains constant
- B. Products are continuously being formed
- C. The rate of forward and backward reactions are the same
- D. The reaction has stopped completely
Explanation
he incorrect statement is: "The reaction has stopped completely." In a state of dynamic equilibrium, the forward and backward reactions are occurring at the same rate. While the macroscopic concentrations of the reactants and products remain constant, this does not imply that the reaction has stopped. On the contrary, at equilibrium, both the forward and backward reactions continue, but their rates are equal. This means that while reactants are being converted into products, products are also converting back into reactants at an equal rate, resulting in a constant overall concentration of reactants and products.
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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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