Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction rate constant 2NO(g) → N₂O₂(g) 2 N₂O₂(g) + O₂(g) 2 NO₂(g) Suppose also k₁ »k₂. That is, the first step is much faster than the second. step 1 Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K₂, and (if necessary) the rate constants k.1 and k.2 for the reverse of the two elementary reactions in the mechanism. 00 rate=& k = 0 k₁ k ローロ 00 X 2 S
Suppose the formation of nitrogen dioxide proceeds by the following mechanism: elementary reaction rate constant 2NO(g) → N₂O₂(g) 2 N₂O₂(g) + O₂(g) 2 NO₂(g) Suppose also k₁ »k₂. That is, the first step is much faster than the second. step 1 Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K₂, and (if necessary) the rate constants k.1 and k.2 for the reverse of the two elementary reactions in the mechanism. 00 rate=& k = 0 k₁ k ローロ 00 X 2 S
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.7: Reaction Mechanisms
Problem 11.12E
Related questions
Question
![Suppose the formation of nitrogen dioxide proceeds by the following mechanism:
elementary reaction
2 NO(g) N₂O₂(g)
2 N₂O₂(g) + O₂(g) 2 NO₂(g)
Suppose also k₁ >>k₂. That is, the first step is much faster than the second.
step
1
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of K₁, K₂,
and (if necessary) the rate
constants k.₁ and k-2 for
the reverse of the two
elementary reactions in
the mechanism.
0
rate = k
k =
rate constant
k₁
k₂
ローロー
00
X
2
S
4](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fad6d3305-3f03-4e1d-b5fa-fcc90cc2dc7c%2F7d0e17d3-f89c-4bd0-9cf9-c72525e169c8%2F4pct2hu_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose the formation of nitrogen dioxide proceeds by the following mechanism:
elementary reaction
2 NO(g) N₂O₂(g)
2 N₂O₂(g) + O₂(g) 2 NO₂(g)
Suppose also k₁ >>k₂. That is, the first step is much faster than the second.
step
1
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of K₁, K₂,
and (if necessary) the rate
constants k.₁ and k-2 for
the reverse of the two
elementary reactions in
the mechanism.
0
rate = k
k =
rate constant
k₁
k₂
ローロー
00
X
2
S
4
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