Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Answer all parts
![Use the following technique and the data below to verify
that the decomposition of nitrogen dioxide is second order.
2NO₂(g) → 2NO(g) + O2(g)
The rate law for the decomposition of nitrogen dioxide can
be written as
Rate = k[NO₂]", or k=
when
n is the order of the reaction. Note that when you divide the
rates at various times by the concentrations raised to the
correct power
n, you should get the same number (the rate constant
k). Divide each average rate in a time interval by the square
of the average concentration in that interval. Note that each
calculation gives nearly the same value. Take the average of
these calculated values to obtain the rate constant.
Time
0.00 min
1.00 min
2.00 min
3.00 min
k₁ =
/(M.s)
k₂ =
/(M.s)
k3 =
/(M.s)
Kaverage =
/(M.s)
[NO₂]
0.3650 M
0.3370 M
0.3126 M
rate
[NO₂]"
0.2935 M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2Fd3f5c130-4632-458d-b2c4-3c75c2e284a6%2Fdf5hhi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Use the following technique and the data below to verify
that the decomposition of nitrogen dioxide is second order.
2NO₂(g) → 2NO(g) + O2(g)
The rate law for the decomposition of nitrogen dioxide can
be written as
Rate = k[NO₂]", or k=
when
n is the order of the reaction. Note that when you divide the
rates at various times by the concentrations raised to the
correct power
n, you should get the same number (the rate constant
k). Divide each average rate in a time interval by the square
of the average concentration in that interval. Note that each
calculation gives nearly the same value. Take the average of
these calculated values to obtain the rate constant.
Time
0.00 min
1.00 min
2.00 min
3.00 min
k₁ =
/(M.s)
k₂ =
/(M.s)
k3 =
/(M.s)
Kaverage =
/(M.s)
[NO₂]
0.3650 M
0.3370 M
0.3126 M
rate
[NO₂]"
0.2935 M
Transcribed Image Text:Nitrogen monoxide reacts with oxygen gas to form nitrogen dioxide.
2 NO(g) + O₂(g) → 2 NO₂(g)
Determine the rate law for the following mechanism.
Step 1, Fast equilibrium NO(g) + O₂(g) → OONO(g)
Step 2, Slow
NO(g) + OONO(g) → 2 NO₂(g)
Rate =
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