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

Option (b) is correct

Step-by-step 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-
`(1)/([A])=(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
`(1)/([A])` is y and t is x.

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

`rate = k[X]^(2)`