I have a question about calculating rates and determining orders:
Three runs were used to study the reaction: A + B :rarrow:C + D
The following data was obtained (initial concentrations of C and D = 0
Initial Conentration (M)
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Run [A] [ B]
1 3.000 2.000
2 6.000 2.000
3 3.000 4.000
Concentration after 150 s (M) (I had to fill out this table based on the reaction stoichiometry)
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Run [A] [ B] [C]
1 2.970 1.970 0.09
2 5.940 1.940 0.18
3 2.880 3.880 0.360
(?) Calculate the rate in M/s for each of the three runs.
I know that Rate=-1/a x Δ[A]/Δt
But I do not know what values to substitute.
Also, when I'm finding the order, do I first write the rate law expression, choose 2 sets of data that depend on one reactant while the rest are held constant, set up ratio of rates, and take the log of the expression?