1. The gas phase reaction of nitric oxide and oxygen yields nitrogen dioxide: 2 NO(g) + O₂(g) 2 NO₂ (g) The rate law is rate = K[NO]²[0₂]. a. What is the reaction order with respect to each reactant and what is the overall reaction order? b. What are the units for kif time was expressed in units of minutes? c. If the concentration of NO was doubled and the concentration of O₂ was halved, what would happen to the rate? d. If the NO was unchanged and the concentration of O₂ was doubled, what would happen to the rate? e. If both of the reactants were tripled, what would happen to the rate? 2. The reaction... 2 ICI (9)+ H₂ (9) I2 (g) + 2 HCl (g) is first order in H₂ and first order in ICI. Write the rate law expression and specify the units of the rate constant, k.
1. The gas phase reaction of nitric oxide and oxygen yields nitrogen dioxide: 2 NO(g) + O₂(g) 2 NO₂ (g) The rate law is rate = K[NO]²[0₂]. a. What is the reaction order with respect to each reactant and what is the overall reaction order? b. What are the units for kif time was expressed in units of minutes? c. If the concentration of NO was doubled and the concentration of O₂ was halved, what would happen to the rate? d. If the NO was unchanged and the concentration of O₂ was doubled, what would happen to the rate? e. If both of the reactants were tripled, what would happen to the rate? 2. The reaction... 2 ICI (9)+ H₂ (9) I2 (g) + 2 HCl (g) is first order in H₂ and first order in ICI. Write the rate law expression and specify the units of the rate constant, k.
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.3: Effect Of Concentration On Reaction Rate
Problem 1RC: The reaction NO(g) + 1/2 Cl2(g) NOCl(g) is first-order in [Cl2] and second-order with respect to...
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![1. The gas phase reaction of nitric oxide and oxygen yields nitrogen dioxide:
2 NO(g) + O₂(g)
2 NO₂ (g)
The rate law is rate = K[NO]²[0₂].
a. What is the reaction order with respect to each reactant and what is the overall
reaction order?
b. What are the units for k if time was expressed in units of minutes?
c. If the concentration of NO was doubled and the concentration of O₂ was halved,
what would happen to the rate?
d. If the NO was unchanged and the concentration of O₂ was doubled, what would
happen to the rate?
e. If both of the reactants were tripled, what would happen to the rate?
2. The reaction...
2 ICI (g) + H₂ (g)
ww
I2 (g) + 2 HCl (g)
is first order in H₂ and first order in ICI. Write the rate law expression and
specify the units of the rate constant, k.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd6cc73a6-72c8-4e2b-a22b-5b06a5805dfc%2F4f8b5e15-8de7-4479-b914-f4e007ee6c63%2F41u73dh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. The gas phase reaction of nitric oxide and oxygen yields nitrogen dioxide:
2 NO(g) + O₂(g)
2 NO₂ (g)
The rate law is rate = K[NO]²[0₂].
a. What is the reaction order with respect to each reactant and what is the overall
reaction order?
b. What are the units for k if time was expressed in units of minutes?
c. If the concentration of NO was doubled and the concentration of O₂ was halved,
what would happen to the rate?
d. If the NO was unchanged and the concentration of O₂ was doubled, what would
happen to the rate?
e. If both of the reactants were tripled, what would happen to the rate?
2. The reaction...
2 ICI (g) + H₂ (g)
ww
I2 (g) + 2 HCl (g)
is first order in H₂ and first order in ICI. Write the rate law expression and
specify the units of the rate constant, k.
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