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(NOJ?(0,1. 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%
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(NOJ?(0,1. 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%
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.35PAE: 11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been...
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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%](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f48f9ee-1450-4445-bd34-e2981179c72b%2F7851285a-dd74-423c-929e-3538c364c660%2F7l7b0xc_processed.png&w=3840&q=75)
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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