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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
![22. The decomposition of Brz was followed as a function of time at constant temperature. A plot of In[Brz] vs.
time is shown in the figure below. State the order of this reaction and estimate the rate constant.
-0,5-
-1-
-1.5-
-2-
-2.5-
20
40
60
80
Time (s)
A) first order, -0.03 s
B) first order, 0.03 s
C) first order, 33.3 s!
D) second order, 0.045 M's
E) second order, 22.2 M's!
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In [Br2]](https://content.bartleby.com/qna-images/question/ed3a44e0-c5b9-429c-a420-1377218a2661/82801908-ef35-438f-870b-0bbb44010a8a/i20g6ri_thumbnail.jpeg)
Transcribed Image Text:22. The decomposition of Brz was followed as a function of time at constant temperature. A plot of In[Brz] vs.
time is shown in the figure below. State the order of this reaction and estimate the rate constant.
-0,5-
-1-
-1.5-
-2-
-2.5-
20
40
60
80
Time (s)
A) first order, -0.03 s
B) first order, 0.03 s
C) first order, 33.3 s!
D) second order, 0.045 M's
E) second order, 22.2 M's!
Type here to search
hp
In [Br2]
Expert Solution
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Step 1
The order of the reaction is the sum of exponents of concentration in the rate law equation.
The rate constant, k is the constant that quantifies rate and determines the direction of the reaction.
Step by stepSolved in 3 steps
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
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- 27 The reaction: 2NO + Cl2 → 2NOCl is second order in NO, first order in Cl2 and third order. Compare the initial rate of reaction a mixture of 0.02 mol of NO and 0.02 mol of Cl2 in one liter container with the rate of reaction when two third of NO was consumed? Select one: a. 2/27 b. 3/27 c. 5/27 d. 4/27arrow_forwardThe decomposition of Br2 was followed as a function of time; two different plots of the data are shown here. Part A -0.5 Determine the order and rate constant for the reaction. -1 second order; 0.045 M -1 -1.5 O first order; 33.3 s 1 -2 O second order; 22.2 M '. s 1 -2.5 O first order; 0.030 s1 20 40 60 80 Time (s) Submit Request Answer 10 Provide Feedback 7 2. 20 40 60 80 1/[Brz] In [Brz]arrow_forward
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