HO2(g)+O3(g)-->OH(g)+2O2(g) The rate of this reaction was studied in the presenc

Question

HO2(g)+O3(g)-->OH(g)+2O2(g)

The rate of this reaction was studied in the presence of a large excess of ozone. Determine the psuedo-first-order rate constant and the second-order rate constant for the reaction from the following date:

Pseudo-first-order rate constant= ________________s^-1

Pseudo-second-order rate constant=_______________M^-1

Time [HO2] (M) [O3](M) 0 3.2 x 10^-6 1.0 x 10^-3 10 2.9 x 10^-6 1.0 x 10^-3 20 2.6 x 10^-6 1.0 x 10^-3 30 2.4 x 10^-6 1.0 x 10^-3 80 2.4 x 10^-6 1.0 x 10^-3 HO2(g)+O3(g)-->OH(g)+2O2(g) The rate of this reaction was studied in the presence of a large excess of ozone. Determine the psuedo-first-order rate constant and the second-order rate constant for the reaction from the following date: Pseudo-first-order rate constant= ________________s^-1 Pseudo-second-order rate constant=_______________M^-1

Explanation / Answer

1. Because [B] is in excess we mulitply 99M with 3.67M-1s-1

(99M)(3.67M-1s-1) =  363.33s-1

2. Because [A] is in excess we can mulitply the k' with [A]o to find k

(109M)(45M-1s-1) = 4905s-1   

t1/2 = (ln0.5 / -k)

t1/2 = 1.41 X 10-4s

3. Use the equation [A] = [A]oe-k'[B]ot

(55M) = (99M)e-k'(1000M)(39s)

k' = 1.507 X 10-5M-1s-1

4. Use the equation [A] = [A]oe-k'[B]ot

[A] = (1)e-(0.6 M-1s-1)(45)

[A] = 1.88 X10-12M

5. Use the equation R = k'[A][B]

R = (0.1M-1s-1)(560M)(0.2M)

Rate = 11.2Ms-1

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