Question
e reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
|
exp.
|
[A]/ |
[B]/M |
Initial rate of formation |
|
I |
0.1 |
0.1 |
|
|
II |
- |
0.2 |
4.0 x 10–2
|
|
III |
0.4 |
0.4 |
- |
|
IV |
- |
0.2 |
2.0 x 10–2 |
Solution
Rate law for the reaction is given by:
Rate = k [A]1 [B]0 = k[A]
2.0 x 10–2 mol L–1 min–1 = k[0.1 mol L–1]
Rate constant,
Rate constant = k = 0.2 min–1.
(i) In experiment II Rate = k[A]
(ii) In experiment III
Rate = k[A]
= 0.2 min–1 x 0.4 M
= 0.08 min–1
= 8.0 x 10–2 M min–1
(iii) In experiment IV
Rate = k[A]
Thus the completed table is
|
exp.
|
[A]/ |
[B]/M |
Initial rate of formation |
|
I |
0.1 |
0.1 |
|
|
II |
0.2 |
0.2 |
4.0 x 10–2
|
|
III |
0.4 |
0.4 |
8.0 x 10-2 |
|
IV |
0.1 |
0.2 |
2.0 x 10–2 |
