Question

Determine the rate law, including the values of the orders and rate law constant, for the following reaction using the experimental data provided.

A + B products


Trial [A] [B] Rate
1 0.15 M 0.12 M 1.3 × 10^-2 M/min
2 0.30 M 0.12 M 2.6 × 10^-2 M/min
3 0.15 M 0.24 M 5.2 × 10^-2 M/min

Answer 1

here is what i have so far:
rate= k[A]x[B]y

trial 1/trial 2 :
1.3x10^-2/2.6x10^-2 = k[0.15]^x[0.12]^y/k[0.30]^x[0.12]^y
1.3x10^-2/2.6x10^-2 = [0.15]^x/[0.30]^x
1/2 = [1/2]^x
x=1

trial 1/trial 3 :
1.3x10^-2/5.2x10^-2 = k[0.15]^x[0.12]^y/k[0.15]^x[0.24]^y
1.3x10^-2/5.2x10^-2 = [0.12]^y/[0.24]^y
1/4 = [1/2]^y
y= 2
i just dont understand how to find the constant (k)