Practice ProblemBUILD
The reaction
Want to see the full answer?
Check out a sample textbook solutionChapter 14 Solutions
Chemistry
- One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?arrow_forwardRegular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?arrow_forwardWhen heated, tetrafluoroethylene dimerizes to form octafluorocyclobutane. C2F4(g) C4F8(g) To determine the rate of this reaction at 488 K, the data in the table were collected. Analysis was done graphically, as shown below: (a) What is the rate law for this reaction? (b) What is the value of the rate constant? (c) What is the concentration of C2F4 after 600 s? (d) How long will it take until the reaction is 90% complete?arrow_forward
- Hundreds of different reactions occur in the stratosphere, among them reactions that destroy the Earths ozone layer. The table below lists several (second-order) reactions of Cl atoms with ozone and organic compounds; each is given with its rate constant. For equal concentrations of Cl and the other reactant, which is the slowest reaction? Which is the fastest reaction?arrow_forwardCurrent Attempt in Progress The following reaction is investigated to determine its rate law: 2NO(g) + 2H2(g) → N2(g) + 2H2O(g) Experiments yielded the following results: Initial Concentrations (mol L-1) Initial Rate of Formation of N, (mol L-s-) [NO) [H,1 0.40 x 10-4 0.30 x 10-4 1.0 x 10- 0.80 x 10-4 0.30 x 10-4 4.0 x 10- 0,80 x 10-4 0.60 x 10-4 8.0 x 10- What is the rate law for the reaction? O rate = k [NO][H2]² O rate = k [NO]?[H2] O rate = k (NO]?[H2]? O rate = k (NO][H2] What is the value of the rate constant? k= i x 105 O L mol 1s1 O s-1 O L³mol 3s1 O mol L1s-1 O L² mol-2s 1arrow_forwardComplete the following table for the first order reaction: A → product [A] k (min1) Rate (mol/L min) 0.200 2.0 x 103 (c) (b) 0.0372 0.035 6.82 (a) 7.98 x 103 (a) (b) (c)arrow_forward
- (4) Use the following experimental data to write the rate law and the rate constant for the reaction 2 NO (g) + O2 (g) = 2 NO2 (g) Experiment [NO] (M) [O2] (M) Initial rate (M/s) 1 0.0100 0.0100 0.711 x 10-2 2 0.0100 0.0400 2.84 x 10-2 3 0.0200 0.0100 2.84 x 10-2arrow_forwardThe reactionA + B → productswas found to have the following rate law.Rate = k[A]2[B]3In a particular experiment, by what factor will the rate of the reaction increase when the concentrations of A and B are both doubled. A) More information is necessary B) factor of 12 C) factor of 32 D) factor of 24 E) factor of 3 F) factor of 6arrow_forwardA mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F2 + CIO,→FC102 + F step 2 fast: F+ ClO2 → FCio, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]"[B]"... , where 'l' is understood (so don't write it) for m, n etc.) Rate =arrow_forward
- Part A For a reaction that follows the general rate law, Rate = k[A][B]², what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.00? The rate will decrease by a factor of 1/25.0. O increase by a factor of 5.00. O increase by a factor of 25.0. decrease by a factor of 1/5.00. Submit Request Answer loxt >arrow_forwardThe following data were measured for the reaction 2 NO(g) + Br2(g) ---> 2 NOBr(g) Experiment [NO] (M) [Br2] (M) initial rate (M/s) 1 0.10 0.20 24 2 0.25 0.20 150 3 0.10 0.50 60 4 0.35 0.50 735 (a) what is the rate law for the reaction? (b) what is the overall order of the reaction? Group of answer choices A.) a) r = k[NO]4[Br2]2 b) 6 B.) a) r = k[NO]3[Br2] b) 4 C.) a) r = k[NO]2[Br2] b) 3 D.) a) r = k[NO]2[Br2] b) 2arrow_forwardSuppose the parent reaction: A + 2B AB2 occurs by the following mechanism: Step 1 A + B AB slow Step 2 AB + B AB2 fast The rate law expression of the parent reaction is Rate = (a) k[A][B]2 (b) k[B] (c) k[A][B] (d) none of thesearrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning