Question

For the reaction A+B+C→D+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	9.0×10−5
2	0.30	0.30	0.90	2.7×10−4
3	0.60	0.30	0.30	3.6×10−4
4	0.60	0.60	0.30	3.6×10−4

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

Answer 1

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 .