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]

Respuesta :

Answer:

Option (b) is correct

Explanation:

For a second order of reaction of type:

                                [tex]2A\rightarrow products[/tex]

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

Integrated rate law is-  [tex]\frac{1}{[A]}=\frac{1}{[A]_{0}}+kt[/tex], where [tex][A]_{0}[/tex] 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 [tex]\frac{1}{[A]}[/tex] is y and t is x.

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

                                   [tex]rate = k[X]^{2}[/tex]

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