Consider the following reaction.
4 A + B + 2 C →→ 4 D + E
The following data was collected on the reaction.
Trial | [A]0 | [B]0 | [C]0 | Rate (M/s) |
1 | 0.22 | 0.75 | 0.22 | 9.506 |
2 | 0.44 | 0.75 | 0.22 | 19.012 |
3 | 0.22 | 1.5 | 0.22 | 19.012 |
4 | 0.22 | 0.75 | 0.44 | 9.506 |
Two mechanisms are proposed:
Mechanism 1:
A + B | →→ | D + Y |
Y + C | →→ | X |
X + A + C | →→ | D + Z |
Z + A | →→ | E |
Mechanism 2:
A + C | →→ | D + Y |
Y + B + C | →→ | X + D |
X + A + C | →→ | E |
Which mechanism best fits the data? Select an answer ( Mechanism 1, Mechanism 2 )
Which is most likely the rate-determining step? Select an answer( Step 1 ,Step 2, Step 3, Step 4 )
rate law is
rate = K[A]x[B]y[C]z
from trial 1
rate = 9.506 = K *(0.22)x (0.75)y (0.22)z (1)
from trial 2
rate = 19.012 = K* (0.44)x *(0.75)x(0.22)z (2)
trial 3
rate = 19.012 = K *(0.22)x ( 1.5)y (0.22)z (3)
trial 4
rate = 9.506 = K*(0.22)x(0.75)y(0.44)z (4)
now, trial 1/ trial 4
(0.22)/(0.44)z = (9.506/9.506) = 1
or, Z = 0.
trial 1/trial 2
(0.22)x/(0.44)x = (9.506/19.012) = (1/ 2)
or, X = 1
trial 1/ trial 3
(0.75/0.15)y = (9.506/19.012) = (1/2)
or, Y = 1
then rate law is
rate = K*[ A] [B]
overall order = (1+1) = 2
so, rate of the reaction is independent on concentration of C.
In mechanism 2, in all the steps C is present. But in mechanism 1 , C is not present in all the steps.
Hence, mechanism 1 , best fits the data.
rate of the reaction depends on the slowest step.
By rate law the rate of the reaction depends only on the concentration of A and B, so rate-determining step is step 1.
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