Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A.
[A](M) Initial Rate (M/s)
0.15 0.011
0.30 0.044
0.60 0.177

What is the order of the reaction?Express your answer as an integer.

Write a rate law for the reaction.Rate=k[A]3Rate=kRate=k[A]Rate=k[A]2

(1) order = 2

(2) R = K [A]²

Explanation:

Given the reaction:

A>Product

The rate constant relation for the reaction is given as:

R(i) = K [A](*)

Where R(I) is rate constant at different concentration of A.

Taking the rate constant as R1, R2 and R3 for the different concentrations respectively. Then the following equations results

0.011 = K [0.15] ⁿ(1)

0.044 = K [0.30]ⁿ (2)

0.177 = K [0.60]ⁿ (3)

Dividing (2) by (1) and (3) by (1)

Gives:

0.044/0.011 = [0.3/0.15]ⁿ

4 = 2ⁿ; 2² = 2ⁿ; n = 2

Similarly

0.177/0.011 = [0.60/0.15]ⁿ

16.09 = 4ⁿ

16.09 = 16 (approximately)

4² = 4ⁿ ; n = 2

Hence the order of the reaction is 2.

The rate law is R = K [A]²

Step-by-step explanation:

the 2nd line can be rewritten as y < x-3

So, any value that is less than both 4x+4 and x-3 will work

Pick any value you want for x, and figure y possibilities

x=0; x-3=-3, 4x+4=4, so y<-3 ... (0,-5) will work

I'm sure you can now come up with other pairs.