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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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13.63
![Review Intelligent Tutoring Question 13.63
The oxidation of NO (released in small amounts in the exhaust of automobiles) produces the brownish-red gas NO, which is a component of urban air pollution.
2NO + 02
ZNO,
The rate law for the reaction is
rate = K[NO)°(0,). At 25°C, k = 7.1 x 10° L?mor?s.
What would be the rate of the reaction if
(NO] = 0.0010 mol L and
(0,) = 0.034 mol L?
rate =
mol Ls!
the tolerance is +/-2%](https://content.bartleby.com/qna-images/question/7f48f9ee-1450-4445-bd34-e2981179c72b/7851285a-dd74-423c-929e-3538c364c660/7l7b0xc_thumbnail.png)
Transcribed Image Text:Review Intelligent Tutoring Question 13.63
The oxidation of NO (released in small amounts in the exhaust of automobiles) produces the brownish-red gas NO, which is a component of urban air pollution.
2NO + 02
ZNO,
The rate law for the reaction is
rate = K[NO)°(0,). At 25°C, k = 7.1 x 10° L?mor?s.
What would be the rate of the reaction if
(NO] = 0.0010 mol L and
(0,) = 0.034 mol L?
rate =
mol Ls!
the tolerance is +/-2%
Expert Solution
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Step 1
Given:
Formula:
The given rate equation for the reaction is:
Where,
k= rate constant
[NO]= Concentration of NO
[O2]= Concentration of O2
To find:
Rate
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