Question

# For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants....

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: 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 .