Connect for Chemistry
13th Edition
ISBN: 9781260161854
Author: Raymond Chang, Jason Overby
Publisher: Mcgraw-hill Higher Education (us)
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Textbook Question
Chapter 13.5, Problem 2RCF
For the reaction between NO and O2, the following mechanism has been suggested:
What is the rate law for this reaction?
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Students have asked these similar questions
The formation of dinitrogen pentoxide is described by the following chemical equation:
2NO, (g) + O; (g) → 0, (g) + N,O5 (g)
Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction:
NO2 (g) + 03 (g) NO; (g) + 0,
Suppose also that the second step of the mechanism should be bimolecular.
Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed
mechanism.
Phosgene (COCI) reacts with formaldehyde in the following reaction to produce dichloromethane and
carbon dioxide:
CoCI, + CH;0 → CH;Cl, + CO,
P+F>D+C
Activated charcoals have been found to catalyse this reaction at 170 °C (Ryan & Stacey, 1984).
One possible mechanism by which the reaction is thought to occur is shown below:
P+s = P.S
Egn 1
P.S + Fie
1.
C.S +D Egn 2
C.S
C+S
Egn 3
a) What type of reaction is Eqn 2 in the mechanism?
b) Write rate expressions (aka rate law aka isotherms) for all the reactions.
c) What do you believe would be the rate limiting step? Use this to derive the rate law for the reaction.
d) What is the best way to confirm the rate law you derived theoretically in c)?
Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism:
step
elementary reaction
rate constant
1
NO2(g) + O3(g)
→
NO3(g) + O₂(g)
k₁
2
NO3(g) + NO₂(g) → N₂O5(9)
k₂
Suppose also k₁«k₂. That is, the first step is much slower than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
0
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.
rate = k
k = 0
Chapter 13 Solutions
Connect for Chemistry
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