-1 -1 products, k 0.379 M' s. If the initial concentration of 56. For the hypothetical second-order reaction A A is 0.799 M, how long would it take for A to be 39.7% consumed? a. 5.01 s b. 3.3129 s c. 1.33 s d. 2 s e. 2.43 s
-1 -1 products, k 0.379 M' s. If the initial concentration of 56. For the hypothetical second-order reaction A A is 0.799 M, how long would it take for A to be 39.7% consumed? a. 5.01 s b. 3.3129 s c. 1.33 s d. 2 s e. 2.43 s
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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![18 / 37
106%
56. For the hypothetical second-order reaction A
A is 0.799 M, how long would it take for A to be 39.7% consumed?
-1
If the initial concentration of
products, k= 0.379 Ms.
a. 5.01 s
b. 3.3129 s
c. 1.33 s
d. 2 s
е. 2.43 s
57. Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction
N204(g)
→2NO,(g)
At 400.0 K, the rate constant for this reaction has been measured to be 2.9 x 10° L/(mol s). Suppose
0.742 mol of N2O4(g) is placed in a sealed 34.3-L container at 400.0 K and allowed to react. What is
the total pressure inside the vessel after 49.6 ns has elapsed? (R= 0.0821 (L atm)/(K mol))
a. 0.879 atm
b. 0.7138 atm
c. 0.541 atm
Type here to search
6ODA](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3722bb55-5371-427b-8e97-5980ded962b0%2Ff7e1f988-ee79-49e0-b49a-9ee905ae4d8e%2Fxlkw5ie_processed.jpeg&w=3840&q=75)
Transcribed Image Text:18 / 37
106%
56. For the hypothetical second-order reaction A
A is 0.799 M, how long would it take for A to be 39.7% consumed?
-1
If the initial concentration of
products, k= 0.379 Ms.
a. 5.01 s
b. 3.3129 s
c. 1.33 s
d. 2 s
е. 2.43 s
57. Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction
N204(g)
→2NO,(g)
At 400.0 K, the rate constant for this reaction has been measured to be 2.9 x 10° L/(mol s). Suppose
0.742 mol of N2O4(g) is placed in a sealed 34.3-L container at 400.0 K and allowed to react. What is
the total pressure inside the vessel after 49.6 ns has elapsed? (R= 0.0821 (L atm)/(K mol))
a. 0.879 atm
b. 0.7138 atm
c. 0.541 atm
Type here to search
6ODA
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