1. The problem statement, all variables and given/known data Data in the table were collected at 300 K for the following reaction: A(g) + B(g) → products Concentration of A 1.00 0.100 1.100 Concentration of B 0.100 0.100 1.00 Initial Rate (M/s) 1.29x10^-29 1.33x10^-30 1.30x10^-29 Determine the rate law for the reaction. 2. Relevant equations Rate = k[A]^m^n, where m and n are the reaction orders. 3. The attempt at a solution I tried to find the factor [A] increases by for trials 1 and 2, and got the value 0.1. I got a value of 0.103 for the rate that the initial rate changes from trial 1 to 2. From there, I get stuck. I had an equation that I used to try and find the reaction order for [A], but I cant seem to find it anywhere, and any other attempts to find the reaction order give me negative values such as -6, and impossibly large numbers. Please help! Also, for some reason I cant see the homework template that keeps getting suggested to me. Is there a pdf download anywhere?