Q. 17

Compounds ‘A’ and ‘B’ react according to the following chemical equation.

A (g) + 2 B (g) 2C (g)

Concentration of either ‘A’ or ‘B’ were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.


A. Rate = k [A]2 [B]

B. Rate = k [A] [B]2

C. Rate = k [A] [B]

D. Rate = k [A]2 [B]0

Answer :

We know that the

Rate=k[A]x[B]y


To determine the value of x and y, We will use the data given in the table


By observing that when the concentration of B is doubled keeping the molar concentration of A constant the rate of production of C changes from .10 to .40, it means then the rate of production of C or Rate is directly proportional to the square of the molar concentration of B.


By keeping the concentration of B constant and on doubling the concentration of A from .30 to .60, the rate of production of C changes from .1 to .2, this means that the rate of production of C or Rate is directly proportional to the molar concentration of A.


Hence, x=1 and y=2,


Rate=k[A][B]2


The value of x and y, for the other options, do not give the correct value rate of production of C for the respective value of A and B.

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