For the reaction A+B+CD+E, the initial reaction rate was measured for various in
ID: 979523 • Letter: F
Question
For the reaction A+B+CD+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected:
Trial
[A]
(M)
B]
(M)
[C]
(M)
Initial rate
(M/s)
1
0.30
0.30
0.30
9.0×105
2
0.30
0.30
0.90
2.7×104
3
0.60
0.30
0.30
3.6×104
4
0.60
0.60
0.30
3.6×104
rate=k[A]^m[B]^n
What is the value of the rate constant k for this reaction?
Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash
Trial
[A]
(M)
B]
(M)
[C]
(M)
Initial rate
(M/s)
1
0.30
0.30
0.30
9.0×105
2
0.30
0.30
0.90
2.7×104
3
0.60
0.30
0.30
3.6×104
4
0.60
0.60
0.30
3.6×104
Explanation / Answer
Answer: Here first we have to calculate the order of the reaction .
Now considering equation 1 and 3 we get :
9.0 * 10-5/3.6 * 10-4 = [0.30/0.60] m
1/4 = 1/2]m
now we get the value of m is 2 .
now consedering data 3 and 4 we get
3.6 * 10-4 / 3.6 * 10-4 = 1/2]n
1= 1/2]n
hence vale of n is 0
Now we can use the formula to calculate the value of K
from data 4: 3.6 * 10-4 = K [ 0.60]2
And we get rate constant value 10-3
Hence the required answer is 10-3 .
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