Chemistry: Atoms First
18th Edition
ISBN: 9781938168154
Author: Richard Langley, Klaus Theopold, Paul Flowers
Publisher: OpenStax College
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Textbook Question
Chapter 17, Problem 31E
The following data have been determined for the reaction:
1 | 2 | 3 | |
|
0.10 | 0.20 | 0.30 |
|
0.050 | 0.050 | 0.010 |
Rate(mol/L/s) |
|
|
|
Determine the rate equation and the rate constant for this reaction.
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The following reaction was analyzed and data was collected.
3 A (g) + 2 B4 (g) + C2 (g) – D (g)
Initial Concentration (mol L)
(Ba]
0.100
Trial
Initial Rate
(mol Ls4)
9.072 x 109
3.629 x 10
2.449 X 107
3.135 х 10%
[A]
[C:]
1
0.100
0.400
2.
0.400
0.100
0.400
0.100
0.300
0.400
4
0.100
0.600
1.60
0.600
0.75
0.100
a) Determine the rate law and rate constant for the reaction. Be sure to show all of your work.
b) Determine the rate for the fifth reaction.
The rate of a chemical reaction depends on the
concentrations of the reactants. Let's consider the
general reaction between A and B:
aA + bB = cC + dD
The dependence of the reaction rate on the
concentration of each reactant is given by the
equation called the rate law.
n
rate = k[A]" [B]"
where k is a proportionality constant called the rate
constant. The exponent m determines the reaction
order with respect to A, and n determines the
reaction order with respect to B. The overall
reaction order equals the sum of the exponents (
m+n).
For example, if m = 2 andn=2 then
rate = k[A]2 B]² and the overall reaction order is
2+2=4.
The reaction orders are experimentally determined
and usually not related to the reaction
stoichiometric coefficients a and b.
Given the experimental data of CO + NO2 → CO2 + NO,
Initial
Initial
Initial Rate
Experiment
[CO]
[NO2]
of Reaction
(M)
(M)
(M/s)
1
0.005
0.040
3.4 x 10-8
2
0.005
0.020
1.7 x 10-8
3
0.010
0.040
6.8 x 10-8
Write the rate law expression for the reaction, the overall order of reaction; and calculate the rate constant (k).
Chapter 17 Solutions
Chemistry: Atoms First
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