4. Ozone decomposes to molecular oxygen according to the following balanced reac

Question

4. Ozone decomposes to molecular oxygen according to the following balanced reaction: 2O3 3O2, described by the rate law: rate = k[O3]2. a) What is the relationship between d[O3]/dt , d[02]/dt and the rate of the reaction as written above. b) In certain cases the rate of the loss of one mole of O3 is of interest, so the relevant balanced reaction would be: O3 - 3/2O2. If we call the rate constant for this reaction k': i. What is the rate law for the reaction O3 - > 3/2O2 ii. What is the relationship between k and k'.

Explanation / Answer

2O3..........> 3O2

a)

rate = -1/2d[O3]/dt = +1/3 d[O2]/dt

b)
i)
rate law can not depends on the balnced equation . it is experimental one.

so the rate law ==> rate =K'[O3]^2

ii)
K = K'

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