🏷️ LIMITED TIME OFFER: GET 20% OFF GRADE+ YEARLY SUBSCRIPTION →
Log in
Chemistry
2
answers
0
watching
280
views

Consider the second-order reaction: 2NO2(g) ---> 2NO (g) +O2(g)

Find the initial concentration [NO2]0 and the rate constant k forthe reaction. What will be the concentration of NO2 after t = 30.0s([NO2]t) for a reaction with this information:

Rate law: k[NO2]2
k=.541/(mol/s) at 573k
initial rate= 1.35 mol/(ls)
rate=0.13 mol/(ls)
[NO2]= 0.49 mol/l

Watch
2
answers
0
watching
280
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
Hubert Koch
Hubert KochLv2
28 Sep 2019
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Consider the second-order reaction:

2NO2(g)?2NO(g)+O2(g)

Use the simulation to find the initial concentration [NO2]0 and the rate constant k for the reaction. What will be the concentration of NO2 after t = 40.0s
([NO2]t) for a reaction starting under the condition in the simulation?

At a certain temperature the following data were collected for thereaction:
4 NO2(g) + O2(g) --------> 2 N2O5(g)

[NO2](M) [O2](M) Initial rate (M/s)
0.0250 0.0110 3.10*10^-4
0.0250 0.0220 6.20*10^-4
0.0500 0.0110 6.20*10^-4


What is the rate law for this reaction?

a) rate = k[NO2][O2]

b) rate = k[NO2]2[O2]2

c) rate = k[NO2]

d) rate = k[NO2]0.5[O2]

What is the value of the rate constant for the reaction?
_________________L•mol-1•s-1 ?


Characteristics of second-order reactions
For a second-order reaction, [A]?products, the rate of the reaction is given as rate= k[A]2, where k is the rate constant and [A] is the concentration of reactant A. The integrated rate law for second-order reactions is 1[A]t=kt+1[A]0, where [A]t is the concentration of reactant A at time t, k is the rate constant, and [A]0 is the initial concentration of reactant A. This equation is of the type y=mx+b. Therefore, the plot of 1[A]t versus time is always a straight line with a slope k and a y intercept 1[A]0.

Part B
Consider the second-order reaction:

2NO2(g)?2NO(g)+O2(g)

Use the simulation to find the initial concentration [NO2]0 and the rate constant k for the reaction. What will be the concentration of NO2 after t = 40.0s ([NO2]t) for a reaction starting under the condition in the simulation?
Express your answer in moles per liters to three significant figures.


Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in