Question

The following questions refer to the hypothetical reaction A + B  products. The kinetics data given can be analyzed to answer the questions. [A]0 [B]0 Rate of decrease (mol/L) (mol/L) of [A] (M/s) 5.0 5.0 X 10.0 5.0 2X 5.0 10.0 2X Time (s) [B] (mol/L) 10.0 100 20.0 100 30.0 100 62. The rate law for the reaction is Rate = k[A]x[B]y. What are the values of x and y? A) x = 0 y = 1 B) x = 1 y = 0 C) x = 1 y = 1 D) x = 2 y = 1 E) x = 1 y = 2

Answer 1

To determine the rate law for the reaction A + B -> products, we need to examine how the rate of the reaction changes as the concentrations of A and B change. From the given data, we can see that when the concentration of A is doubled, the rate of the reaction also doubles. Similarly, when the concentration of B is doubled, the rate of the reaction also doubles. This indicates that the rate of the reaction is directly proportional to the concentrations of both A and B.

Based on this information, the rate law for the reaction can be expressed as Rate = k[A]*[B], where k is the rate constant. The exponents x and y in the rate law represent the order of the reaction with respect to A and B, respectively. Since the rate of the reaction is directly proportional to the concentrations of both A and B, the exponents x and y would both be equal to 1.

Therefore, the values of x and y are C) x = 1 and y = 1.