Consider the reaction aX bY , for which the rate constant at 30°C is 1 10⁻³ mol ⁻¹ L s ⁻¹ . Which of the following statements are true? A. When concentration of 'X' is increased to four times, the rate of reaction becomes 16 times. B. The reaction is a second order reaction. C. The half-life period is independent of the concentration of X. D. Decomposition of N₂ O₅ is an example of the above reaction. E. [R_o] [R] vs

Step-by-step solution

The unit of the rate constant k is mol ⁻¹ L s ⁻¹ . The general unit of the rate constant for an n -th order reaction is (mol L ⁻¹ ) ^ 1-n s ⁻¹ . Equating the powers of the concentration units, we get 1-n = -1 n = 2 . Thus, the reaction is a second-order reaction. Statement B is correct. For a second-order reaction, Rate = k[X]^2 . When the concentration of X is increased to 4 times, the new rate is k(4[X])^2 = 16k[X]^2 , which is 16 times the original rate. Statement A is correct. The half-life of a second-order re