Question
For the reaction, A+B → Products, it is observed that
1) On doubling the initial concentration of A only, the rate of reaction is also doubled and
2) On doubling the initial concentrations of both A and B , there is a change by a factor of 8 in the rate of the reaction.
The rate of this reaction is, given by
-
rate = k [A]2[B]
-
rate = k[A][B]2
-
rate = k[A]2[B]2
-
rate = k[A][B]
Solution
B.
rate = k[A][B]2
For the reaction,
A +B → product
on doubling the initial concentration of An only the rate of reaction is also doubled, therefore,
..... (i)
Let initially rate law is
Rate = k[A][B]y
If the concentration of A and B both are doubled, the rate gets changed by a factor of 8.
8 x Rate = k[2A][2B]y ...... (iii)
Dividing eq (iii) by eq. (ii),
8 = 2 x 2y
4 = 2y
y=2
Dividing eq (iii) by eq. (ii),
8 = 2 x 2y
4 = 2y
y=2
