The rate law for the reactionNO2(g) + O2(g)is given by rate =-k[NO₂]NO(g) + 03 (g)If the following is the mechanism for the reaction, which of the following statements correctly describe the reaction? Check all that apply.NO2(g) NO(g) + O(g)-O(g) + O2(g) 03 (g)The reaction is 2nd order overall.The first step is the slow step.Doubling NO, would quadruple the rate.Cutting O, in half would decrease the rate by a factor of 2.The molecularity of the first step is 1.Both steps are termolecular.None of the above

To determine which statements correctly describe the reaction based on the given rate law and the…

Answered: The rate law for the reaction NO2(g) +…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?
The reaction 2 H2(g) + 2 NO(g) -> 2 H₂O(g) + N2(g) is first order in H₂ and second order in NO. Write the Rate Law for this reaction.
Given the following data, determine the rate law for the reaction 2NO(g) + Cl2(g) 2NOCI(g) Еxperiment [NO] (M) 0.0300 [Ch] (M) 0.0100 Rate (Mls) 1 3.4 x 10 8.5 x 105 3.4 x 10 0.0150 0.0100 0.0150 0.0400 =K[NO][Ch]. Rate = k[NO][Cll Rate = k[NO] [Ch] Rate = k[NO]°ICl Rate = k[NO][C2]" a. d. %3D b. e. C. e O d O a O b Ос
The reaction 2H2(g) + 2NO(g) ----> 2H2O(g) + N2(g) is a first-order in H2 and second order in NO. What is the rate law
Consider the following reaction: 2 CH3l (aq) C2H6 (g) + 12 (g) This reaction is first-order, and its rate constant, k at 25°C is 0.0115 s¹. a) If the initial concentration of CH3l is 6.75 M, what is the concentration of CH3I after the reaction has been carried out for 1.83 hours? Report your answer using most of the decimal places reported on your calculator. Do not use scientific notation [CH31]= M b) If the rate constant is increased by a factor of 2.36 when the temperature is raised from 25°C to 76.6 °C, what is the activation energy (in kJ/mol) for this reaction? Report your answer using most of the decimal places reported on your calculator. Do not use scientific notation Ea kJ/mol
The reaction 2 NO(9) + 02 (9) → 2 NO2(9) was studied, and the following data were obtained where A[02] Rate = At NOo [02]o Initial Rate (molecules/cm³) (molecules/cm) (molecules/cm° · s) 1.00 x 1018 1.00 x 1018 2.00 × 1016 3.00 x 1018 1.00 x 1018 1.80 x 1017 2.50 × 1018 2.50 × 1018 3.13 x 1017 What would be the initial rate for an experiment where [NO], = 2.66 × 1018 molecules/cm° and [O2]o 1.48 x 1018 molecules/cm°? Rate = |molecules/cm³ . •S
The rate law for the reaction 2NO(g) + Cl2(g) →2NOCl(g) is given by R = k[NO][Cl2] If the following is the mechanism for the reaction, NO(g) + Cl2(g) → NOCl2(g) NOCl2(g) + NO(g) →2NOCl(g) which of the following statements accurately describes this reaction? Check all that apply. 2nd order reaction Both steps are termolecular. The molecularity of the first step is 1. Doubling [NO] would quadruple the rate. Cutting [Cl2] in half would decrease the rate by a factor of two. The first step is the slow step
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)H20(g) + ½ O2(g) is second order in H2O2. In one experiment, when the initial concentration of H,O2 was 0.242 M, the concentration of H,O, dropped to 4.09×10 M after 23.5 seconds had passed. Based on these data, the rate constant for the reaction is M1s1.
Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO₂)² The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1.2A B+C 2. B+D+E+C Part A What is the overall reaction? Express your answer as a chemical equation. ► View Available Hint(s) for Part A for Pardo for Part redo foPart A refor Part A keyboard shortcuts for Part A help for Part A A chemical reaction does not occur for this question. Submit Part B Which species is a reaction…
2 NO (g) + O₂ (g) --> 2 NO2 (g) The proposed mechanism for the reaction above is 1) NO (g) + NO (g) --> N₂O2(g) 2) N₂O2 (g) + O2 (g) --> 2 NO2 (g) Write the rate law for the mechanism if the first step is fast and the second step is slow.
At a certain temperature the rate of this reaction is first order in C1₂O5 with a rate constant of 0.0699 s ! 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) Suppose a vessel contains Cl₂05 at a concentration of 0.910M. Calculate the concentration of C1₂05 in the vessel 11.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
The reaction shown below has the rate law rate=k[NO]2[Cl]. Determine the overall reaction order.2NO(g)+Cl2(g)⟶2NOCl(g) 0 1 2 3

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