Question

# Determine the rate law (be sure to include the value for k) for the following reaction...

Determine the rate law (be sure to include the value for k) for the following reaction using the data provided.

NO2(g)+O3(g)->NO3(g)+O2(g)

[NO2] (M) [O3]i (M) initial rate

0.10 0.33 0.0223

0.10 0.66 0.01788

0.25 0.66 1.112

Please help with reasoning on how to find the order of the reactions when they are not first or 0 order and how to find k. Thank you!

Given reaction is : NO2(g)+O3(g)->NO3(g)+O2(g)

Let the rate law be , r = k[NO2]m [O3]n ----(1)

Where k = rate constant

r = rate of the reaction

m , n = orders of the reaction with respect to NO2 &O3 respectively

Let us apply the above tabulated values to Equation (1) we get

1st values ===> 0.0223 = k[0.10]m [0.33]n ----(2)

2nd values ===> 0.0223 = k[0.10]m [0.66]n ----(3)

3rd values ===> 1.112 = k[0.25]m [0.66]n ----(4)

(4)/(3) gives 49.86 = 2.5m

log 49.86 = m log2.5

m = 4.3

(3) / (2) gives 1 = 2n

---> n = 0

So rate law is r = k[NO2]4.3[O3]0

OR r = k[NO2]4.3

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