Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![(a) Determine the order of the decomposition of N2O5 using the table below, and according to the following balanced chemical equation:
2N2O5 (g) → 2N2O4 (g) + O2 (g)
1
Time (s)
[N2O5] (M)
In [N2O5]
[N2O5]
0.1000
-2.303
10.0
50
0.0707
-2.65
14.1
100
0.0500
-3.00
20.0
200
0.0250
-3.69
40.0
300
0.0125
-4.38
80.0
400
0.00625
-5.08
160.
(b) How did you come to this conclusion?
(c) Determine the rate constant for the reaction.
(d) If this reaction is run in the laboratory under the same conditions, but the initial concentration of N2O5 is 0.375M, what will the concentration of
it be after 3 min (180) s?
(e) What is the half-life of N2O5 in these reactions?
(f) What is the half-life of N2O5 in its decomposition under different conditions, in which it has a rate constant (k = 7.8 × 10-³s)?
B I U A
A
Ix
x X, E E
12pt
Paragraph
P fr](https://content.bartleby.com/qna-images/question/bbeeb476-a64f-4459-b8af-acf5dbdffec4/6f12bf3d-b9f3-4db4-9af8-624286984c96/x8yp2le_processed.png)
Transcribed Image Text:(a) Determine the order of the decomposition of N2O5 using the table below, and according to the following balanced chemical equation:
2N2O5 (g) → 2N2O4 (g) + O2 (g)
1
Time (s)
[N2O5] (M)
In [N2O5]
[N2O5]
0.1000
-2.303
10.0
50
0.0707
-2.65
14.1
100
0.0500
-3.00
20.0
200
0.0250
-3.69
40.0
300
0.0125
-4.38
80.0
400
0.00625
-5.08
160.
(b) How did you come to this conclusion?
(c) Determine the rate constant for the reaction.
(d) If this reaction is run in the laboratory under the same conditions, but the initial concentration of N2O5 is 0.375M, what will the concentration of
it be after 3 min (180) s?
(e) What is the half-life of N2O5 in these reactions?
(f) What is the half-life of N2O5 in its decomposition under different conditions, in which it has a rate constant (k = 7.8 × 10-³s)?
B I U A
A
Ix
x X, E E
12pt
Paragraph
P fr
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