Using the data in the table, determine the rate constant of the reaction and select the appropriate units.

Question

A+2B⟶C+D

Trial[𝐀] (𝐌)	[𝐁] (𝐌)	Rate (M/s)
1	0.360
0.360	0.0224
2	0.360
0.720	0.0224
3	0.720
0.360	0.0896

𝑘= units of k

Answer 1

Your table is not formatted correctly so I'm going with the following data, assuming it is correct.

Trial..........[A] (M)............[B] (M)............Rate (M/s)

1..............0.360...............0.360..............0.0224

2..............0.720...............0.360..............0.0224

3.............0.360................0.720..............0.0896

Comparing trials 1 and 2, we have doulbed [A] keeping [B] constant and the rate did not change

This tells us the reaction is ZERO order in A

Comparing trials 1 and 3, we have doulbed [B] keeping [A] constant and the rate increased by 4 times (from 0.0224 to 0.0896).

This tells us the reaction is 2nd order in B

From this info, we can now write the rate law:

Rate = k[B]²

Using any of the info from the table, we can solve for k:

0.0224 M/s = k [ 0.360 M]²

k = 0.0224 M/s / [0.360 M]²

k = 0.173 M^-1s^-1