Description
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Explanation & Answer
=============================================please find the attachment
=============================================please find the attachment
1. Ozone (O3) is produced in the stratosphere by the chemical reaction shown below. If at a
given instant, molecular oxygen (O2) is reacting at a rate of 2.17 x 10–5 mol/Ls, at what
rate is ozone being produced?
3 O2 (g) 2 O3 (g)
The mole ratio between O2:O3 is 3:2
–5
Reacting rate of O2 = 2.17 x 10 mol/Ls
So the rate of ozone being produced = 2.17 x 10–5 mol/Ls * 2/3
= 1.45 x 10–5 mol/Ls
2. The data below were collected for the reaction at 327 °C: H2 (g) + I2 (g) 2 HI (g)
Experiment
1
2
3
Initial [H2], M
0.113
0.220
0.550
Initial [I2], M
0.110
0.330
0.110
Initial Rate, mol/L•s
3.01 x 10–4
1.76 x 10–3
1.47 x 10–3
a. Determine the rate law for this reaction.
r = K[H2]a[I2]b
b. What is the rate order for [H2], and [I2]? What is the overall rate order for this reaction?
3.01 x 10–4 = k (0.113) a (0.110) b -------------------------(1)
1.76 x 10–3 = k (0.220) a (0.330) b--------------------------(2)
1.47 x10–3 = k (0.550) a (0.110) b ---------------------------(3)
(1)/(3)
0.301/1.47 = (0.113/0.550) a
0.20 = 0.20a
a=1
(1)/(2)
0.301/1.76 =(0.113/0.22)(110/330) b
0.333 = 0.333b
b =1
Rate order for [H2] = 1
[I2] = 1
Overall rate order = 2
c. Calculate the value of k for this reaction and express it with the correct units.
Equa...
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