Question
During the kinetic study of the reaction, 2A + B --> C+ D, following results were obtained
|
|
[A]/mol L- |
[B]/ mol L- |
Initial rate of formation of D/ mol L- min- |
|
I |
0.1 |
0.1 |
6.0 x 10-3 |
|
II |
0.3 |
0.2 |
7.2 x 10-2 |
|
III |
0.3 |
0.4 |
2.88 x 10-1 |
|
IV |
0.4 |
0.1 |
2.40 x10-2 |
based on the above data which one of the following is correct?
-
rate = k[A]2[B]
-
rate = k [A][B]
-
rate = k[A]2[B]2
-
rate = k[A][B]2
Solution
D.
rate = k[A][B]2
Let the order of reaction with respect to A is x and with respect to B is y. Thus,
rate = k[A]x[B]y
For the given cases,
(I) rate = k(0.1)x (0.1)y = 6.0 x 10-3
(II) rate = k (0.3)x (0.2)y = 7.2 x 10-2
(III) rate =k(0.3)x (0.40)y = 2.88 x 10-1
(IV) rate = k(0.4)x (0.1)y = 2.40 x 10-2
On dividing eq. (I) and (IV), we get
