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11 Nov 2019

The rate of the reaction NO2 + CO -> NO +CO2 depends only on the concentration of nitrogen dioxide. The following data was collected

Time (s) [NO2]o, (M)

o .555

1.2 x 10^3 .444

3 x 10^3 .381

4.5 x 10^3 .340

9 x 10^3 .250

1.8 x 10^4 .174

a) determine the rate law

b) write the integrated rate law

c) determine the value of the rate constant for the reaction

d) calculate the [NO2] at 2.4 x 10^4 s after the start of the reaction

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15 Sep 2019

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Related questions

(4) Rate Law from Concentration versus Time Data

NO2(g) + CO(g) --> NO(g) + CO2(g)

The rate of the above reaction depends only on the concentration of nitrogen dioxide at temperatures below 225Â°C. At a temperature below 225Â°C the following data were obtained:

Time (s)

0 1.45Ã10^3

3.62Ã10^3

5.44Ã10^3

1.09Ã10^4

2.18Ã10^4

[NO2] (mol/L)

0.580

0.554

0.519

0.493

0.428

0.340

(a) Which of the following expressions for the rate law (either differential or integrated) are completely consistent with the above experimental data. (say yes or no to each)

1/[NO2] - 1/[NO2]0 = kt

[NO2] = [NO2]0 - kt

ln[NO2] - ln[NO2]0 = -kt

-d[NO2]/dt = k[NO2]^2

k[NO2]^2 = d[CO2]/dt

(b) Calculate the rate constant (k). Enter the numerical value and corresponding units.

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For the reaction 2 NO₂ (g) + F₂ (g) --> 2 FNO₂ (g), initial rate data are listed below. Determine the rate law and solve for the rate constant k (with units), showing all work

Experiment	[NO₂] (M)	[F₂] (M)	[Initial Rate] (M/s)
1	0.0010	0.0020	8.0 x 10^-5
2	0.0020	0.0020	1.6 x 10^-4
3	0.0010	0.0010	4.0 x 10^-5

Rate = _____________ K=_____________ Units:________

What are the rate law and the value of the rate constant for the reaction CO_(aq) + NO_2(aq) CO_2(g) + NO_(g)(using the following data)?

	[CO] (mol/L):	[NO₂] (mol/L):	Initial Rate (mol/Lh):
(1)	5.1 x 10^-4	0.35 x 10^-4	3.4 x 10^-8
(2)	5.1 x 10^-4	0.70 x 10^-4	6.8 x 10^-8
(3)	5.1 x 10^-4	0.18 x 10^-4	1.7 x 10^-8
(4)	1.0 x 10^-3	0.35 x 10^-4	6.8 x 10^-8
(5)	1.5 x 10^-3	0.35 x 10^-4	10.2 x 10^-8