Interpretation:
The rate law for given reaction to be written and simplificationf rate law to be checked, along with the half-lifeaccording to the given conditions, is to be determined.
Concept introduction:
The study of reaction rates, rearrangement of atoms, and the effect of various variables in a
A half-life is the quantity of time it takes for half of a substance to undergo some specified process.
The half-life for the second order reaction is as follows:
The rate law for a chemical reactionis defined as an equation that relates the reaction rate with the concentrations or partial pressures of the reactants.
The rate law is given by:
Answer to Problem 84AP
Solution:
a)
b)
c)
Explanation of Solution
a) The rate law for the reaction
The rate law for a given reaction is as follows:
Here,
It suggests that two molecules of NO are colliding with a molecule of oxygen and forming nitrogen dioxide. This reaction has two or more elementary steps.
Explanation:
b) The rate law can be simplified is to be checked and if so simplified rate law to be written.
A sample of air at a certain temperature is contaminated with
In thegivenreaction, two molecules of
The rate law is given as follows:
Here,
Given information: A sample of air at a certain temperature is contaminated with
Explanation:
c) The half-lifeto be estimated if the initial concentration of NO were 10 ppm
As this reaction is a second-order reaction, the half-life time for this reaction is written as follows:
Here,
The sample is contaminated with
The expression of half-life, by substituting these values in the above equation, can be written as follows:
The initial concentration of
By dividing
Substitute the values of
Therefore, the half-life for an initial concentration of
Want to see more full solutions like this?
Chapter 21 Solutions
ALEKS 360 CHEM ACCESS CARD
- Ozone in the stratosphere can be depleted by the following reactions involving CI atoms: Step 1 (fast): CI + O3 <--> CIO + O2 Step 2 (slow): CIO + O -> CI + O2 (a) What is the rate law according to this mechanism? (b) Based on the rate law from part (b), what should be the units of the observed rate constant, k? Use time units of seconds.arrow_forwardThe overall order of the following reaction 2A + 3B → 2C with the rate law expression: Rate = k[X]1[Y]2 isarrow_forwardThe rate law for a reaction was reported as v= k,[A][B][C] with the molar concentrations in moles per cubic decimetre and the time in seconds. What are the units of k,?arrow_forward
- 11.93 On a particular day, the ozone level in Milwaukee exceeded the EPAs 1-hour standard of 0.12 ppin by 10 ppb. How many ozone molecules would be present in 1 liter of air at the detection site?arrow_forwardThe label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?arrow_forwardWhen boron trifluoride reacts with ammonia, the following reaction occurs: BF3(g)+NH3(g)BF3NH3(g)The following data are obtained at a particular temperature: (a) What is the order of the reaction with respect to BF3, NH3, and overall? (b) Write the rate expression for the reaction. (c) Calculate k for the reaction. (d) When [ BF3 ]=0.533M and NH3=0.300M, what is the rate of the reaction at the temperature of the experiment?arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning