Change in concentration of a reactant is plotted against time and the slope dx/dt determined. The values of dx/dt are plotted against (a-x)2 and a straight line is obtained. It may be concluded that the reaction is:
Correct answer: B. Second order
- A. First order
- B. Second order
- C. Third order
- D. Zero order
Explanation
Option B is correct, indicating that the reaction is second order.When the rate of change of concentration with respect to time, dx/dt, is plotted against (a-x)2 (where 'a' is the initial concentration), and a straight line is obtained, it implies that the reaction follows second-order kinetics.This is a characteristic behavior of second-order reactions. In second-order reactions, the rate is directly proportional to the square of the concentration of a single reactant, which leads to a linear relationship when plotted against (a-x)2.Options A, C, and D are incorrect because they suggest different orders of reaction, which are not consistent with the observed behavior in this scenario.
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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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