Need solution urgently A reaction of importance in the farmation of smog is that between ozone and nitrogen monoxide described by0,+ NO(g) - 0,) + NO, ()The rate law for this reaction israta of reaction = A (0,I[NO]Given that A4.43 x 10 Ms at a certain lenmperature, caleulate the initial reaction rate when (0,1 and (NOJ remainessentially constant at the values 10,- 1.22 x 10M and [NOlo = 7.65 x 10 M, owing to continuous production fromseparate sourcesinitial reaction rate:MCalculate the number of moles of NO, () produced per hour per liter of air.NO, produced:mol hL

Speed of reaction is measured in terms of rate of reaction Here We are required to find the intital…

A reaction of importance in the formation of smog is that between onone and nitrogen monotide descnbed by 0,+ NO(2) 0,R} + NO,(2) The rate law for this reaction is rate of reaction = A (0,1[NO]| Given that A 4.43 x 10 M ata certain lemperature, calculate the initial reaction rate when [0,1 and (NOJ remain esentially constant at the values (0,b-1.22 x 10* M and [NO = 765 x 10 M, owing to continuoun production from separate sources M initial reaction rate: Calculate the number of moles of NO, produced per hour per liter of air. mol h NO, produced

A reaction of importance in the formation of smog is that between onone and nitrogen monotide descnbed by 0,+ NO(2) 0,R} + NO,(2) The rate law for this reaction is rate of reaction = A (0,1[NO]| Given that A 4.43 x 10 M ata certain lemperature, calculate the initial reaction rate when [0,1 and (NOJ remain esentially constant at the values (0,b-1.22 x 10* M and [NO = 765 x 10 M, owing to continuoun production from separate sources M initial reaction rate: Calculate the number of moles of NO, produced per hour per liter of air. mol h NO, produced

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 17E: Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft...

See similar textbooks

Similar questions

Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
The 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,?
a. Express the rate in terms of change of concentration of A with respect to time where 2A + B -> products, rate = k[A]-1. b. Give the derived integrated rate law.
For the rate law Rate = k[A][B]3/2, the order with respect to A is __________, the order with respect to B is __________, and the overall reaction order is __________.
Derive the integrated form of a third-order rate law v = kr[A]2[B] in which the stoichiometry is 2 A +B −−→ P and the reactants are initially present in (a) their stoichiometric proportions, (b) with Bpresent initially in twice the amount.
a. Express the rate in terms of change of concentration of A with respect to time where 2A + B -> products, rate = k[A]-1. b. Give the derived integrated rate law. c. What is the derived expression for half-life with respect to A in terms of k and [A]o?
The rate equation for the reaction A→B + C is expressed in the forms of rate of disappearance of A = k[A]x. The value of the rate constant is 0.100(units unspecified) and [A]= 0.050 mol/L. What are the units of k and the rate reactions in mol/L-s if the reaction is second order?
A certain first-order reaction has a rate constant of 1.50×10−3 s−1s−1. How long will it take for the reactant concentration to drop to 1818 of its initial value? Express your answer with the appropriate units.
The rate constant for the fi rst-order decomposition of N2O5 in the reaction 2 N2 O5(g) → 4 NO2(g) + O2(g) with v = kr[N2O5] is kr = 3.38 x 10-5 s-1 at 25 oC. What is the ha lf- life of N2O5? What w ill be the total pressure, init ial ly 78.4 kPa for the pure N2O5 vapour, (a) 5.0 s, (b) 5.0 min after init iation of the reaction?
A bimolecular chemical reaction is one in which two chemicals react to form another substance. Suppose that one molecule of each of the two chemicals reacts to form two molecules of a new substance. If x represents the number of molecules of the new substance at time t, then the rate of change of x is proportional to the square of the numbers of molecules of the original chemicals available to be converted. That is, if each of the chemicals initially contained A molecules, then dx dt = k(A − x)2 where k is a constant. If 40% of the initial amount A is converted after 1 hour, how long will it be before 50% is converted? (Give an exact answer. Do not round.)
What are the significance of the value of the slope, the value of the y-intercept, and the correlation coefficient to the determination of half-life?
Show that the ratio t1/2/t3/4, where t1/2 is the half-life and t3/4 is the time for the concentration of A to decrease to 3/4 of its initial value (implying that t3/4 < t1/2), can be written as a function of n alone, and can therefore be used as a rapid assessment of the order of a reaction.