Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) N,0(g) + H2O(g) 2 H,(9) + N,0(9) N,(9) + H,O(9) k2 → Suppose also k,«k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U 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 k = the reverse of the two elementary reactions in the mechanism.
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) N,0(g) + H2O(g) 2 H,(9) + N,0(9) N,(9) + H,O(9) k2 → Suppose also k,«k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U 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 k = the reverse of the two elementary reactions in the mechanism.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 105QRT
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Question
![Suppose the reduction of nitric oxide proceeds by the following mechanism:
step
elementary reaction
rate constant
1 H,(g) + 2 NO(g) →
N,0(g) + H,0(g)
k1
2
H2(9) + N,0(9) → N2(9) + H,O(g)
Suppose also k, «k,. That is, the first step is much slower than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
rate = k U
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
k =
the reverse of the two
elementary reactions in
the mechanism.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F36e9e6bf-5fca-412d-926f-13eedac0d9c5%2Fd1cbc351-87a3-4be9-9a47-77ff53d74b4e%2F0b5cg3_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose the reduction of nitric oxide proceeds by the following mechanism:
step
elementary reaction
rate constant
1 H,(g) + 2 NO(g) →
N,0(g) + H,0(g)
k1
2
H2(9) + N,0(9) → N2(9) + H,O(g)
Suppose also k, «k,. That is, the first step is much slower than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
rate = k U
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
k =
the reverse of the two
elementary reactions in
the mechanism.
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