Can anyone help me with this Chemistry Question?

Question

Answer 1

a) rate = k[CO]ⁿ[Cl₂]^m

b) Compare the first 2 lines where [CO] doubles and [Cl₂] remains constant. The rate increases 4x. This tells us that the reaction is SECOND ORDER in CO. Compare line 1 and 3. The [CO] increases 3 fold and the [Cl₂] increases 1.25 times. Based on the reaction being 2nd order in CO, we'd expect the rate to increase 9 fold. The rate actually increases 11.25 fold (0.07425 / 0.00660). Therefore we can find the order with respect to Cl₂ as ...

(3)²(1.25)^m = 11.25

m= 1 so FIRST ORDER in Cl₂

The reaction is THIRD ORDER OVERALL

c) To find the rate constant k, choose any line from the table and plug in the values and solve for k

Using line 1 we have

6.60x10^-3 M/s = k (0.150 M)²(0.100 M)

6.60x10^-3 M/s = k (0.00225 M³)

k = 6.60x10-3 Ms^-1 / 2.25x10^-3 M³

k = 2.93 M^-2s^-1

This was actually a fun problem. I hope that I explained it well enough that you understand the process and that you can do it yourself the next time.