PLEASE HELP I NEED TO SUBMIT THIS HOMEWORK TOMORROW, KINDLY SHOW ALL WORKINGS AN

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PLEASE HELP I NEED TO SUBMIT THIS HOMEWORK TOMORROW, KINDLY SHOW ALL WORKINGS AND CALCULATIONS!!!!! THANK YOU

1. The following reaction was studied at 656 K, and the data below were obtained:

                            2 NO2(g) ? 2 NO(g) + O2(g)

0.0031

a) what is the order of the reaction?

b) What is the rate law?

c) What was the initial concentration of NO2?

d) What is the rate constant?

e) What is the half life?

2. The following reaction was studied in three separate experiments, and the data below were obtained:

                                   2 NO (g) + O2 (g) ? 2 NO2 (g)

a) What is the rate law for the reaction?

b) What is the order of the reaction?

c) What is the rate constant for the reaction?

d) What are the units of the rate constant?

3. The decomposition of hydrogen bromide on a gold catalyst at 120 oC is zero order with respect to HBr. The rate constant is 7.40 x 10-5 M/s.

2 HBr(g) ? H2(g) + Br2(g)

a) Write the rate law for this reaction.

b) If the initial concentration of HBr is 0.870 M, calculate [HBr] after 45 minutes.

4. The following two step mechanism has been proposed for the reaction:

            Overall:          2 NO(g) + H2(g) ? N2O(g) + H2O(g)

            1st step:         NO(g) + NO(g) ? N2O2(g)

            2nd step:        N2O2(g) + H2(g) ? N2O(g) + H2O(g)

a) Show that the elementary steps of the proposed mechanism add up to provide the balanced equation for the reaction.

b) Write a rate law for each step of the reaction.

1st step:

2nd step:

c) List all intermediates in the reaction.

d) If the first step was known to be much slower than the second step, what is the rate law for the reaction?

Time (min) [NO2] 5.00 0.0142 10.0 0.0083 15.0 0.0058 20.0 0.0045 25.0 0.0037 30.0

0.0031

Explanation / Answer

Q1. a)The order of the reaction calculated by initial rate method is 1

using (rate)i =k [NO2]^a

b) The rate law for 2NO2(g) ====> 2NO(g) + O2(g) is rate=k[NO2]^2

c) Initial concentration of [NO2]

rate = -1/2d[NO2]/dt

0.00059 = -1/2[0.0142-[NO2]o]/[5-0]

0.0201 mol/min = [NO2]o

d) rate constant K = ?

First we will find rate = -1/2 d[NO2]/dt = -1/2 [0.0083-0.0142]/[10-5] = 0.00059 mol/min

Now put rate in above equation to find K

rate=k[NO2]^2

0.00059 = k [0.0201] [0.0201]

k = 1.4603

e) Half life of reaction

   t1/2 = 0.693/k

t1/2 = 0.4745

  

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