Question

For the reaction X + Y → Z, the reaction rate is found to depend only upon the concentration of X. A plot of 1/X verses time gives a straight line. Picture What is the rate law for this reaction?

a. rate = k [X]
b. rate = k [X]2
c. rate = k [X][Y]
d. rate = k [X]2[Y]

Answer 1

Answer:

Option (b) is correct

Explanation:

For a second order of reaction of type:

                                $2A\rightarrow products$

Rate law is -  $rate = k[A]^{2}$, where k is rate constant and [A] is concentration of A

Integrated rate law is-  $\frac{1}{[A]}=\frac{1}{[A]_{0}}+kt$, where $[A]_{0}$ is initial concentration of reactant A and [A] is concentration of A after "t" time (k and [A]_{0}[/tex] are constants)

The integrated rate law can be compared with y= mx+c equation for a straight line (x vs y) where $\frac{1}{[A]}$ is y and t is x.

As the rate of reaction depends only upon concentration of X therefore-

                                   $rate = k[X]^{2}$