Can anyone help?
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 yields 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

Question

Can anyone help?
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 yields 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

jfraser · Answer

the general rate law will be$$R = k*[A]^m*[B]^n$$ which is a problem because you've got 3 unknowns: the value of k, the power "m", and the power "n".

By taking 2 different reactions and dividing one rate equation by the other, we can get some terms to cancel.

jfraser · Answer

in 2 of the trials, the concentration of A was kept constant, and B was doubled. In 2 different trials, the concentration of B was kept constant and A was doubled. Use those 2 equations and divide one rate law by the other to make some of those terms disappear