The following was given for a reaction.. (rate law help!!)

A, M B, M RATE M/S
0.1 0.1 5X 10^-4
0.2 0.1 10X10^-4
0.4 0.1 20 X 10^ -4
0.2 0.2 10 X 10^-4
0.2 0.3 10 X 10^-4


That table is given. it asks for the rate law, reaction orders for a and b, and over all reaction order.
Also, what is the average rate constant for the reaction.

We start with rate=K[a]^m[b]^n
To find the order of A you take trail 2 and divide it by trial one K[0.2][0.1] / K[0.1][0.1] = 2^m
divide the rates the same way 10x10^-4 / 5x10^-4= 2
2^m=2 M=1(first order0
To find the order of A you take trail 5 and divide it by trial 4 K[0.2][0.3] / K[0.2][0.2] = 1.5^m
Divide the rates the same way 10x10^-4 / 10x10^-4= 0
This is clearly zero order.
So
rate=K[A]^1[B]^0
Average rate is plug and chug
Find k fore each of these reactions, and average them. Show work, your teacher will probably nail you for not showing your work on this, I know mine would.
I hope it helps.

When you look at the table look for a common trend, as A doubles so does the rate however when A stays the same and B is changed it has no effect on the rate. So the rate is entirely dependant upon A

therefore you can write that rate = k[A], i think this is how it is expressed it is a while since i did this stuff but the reasoning behind it is correct.