Order and rate law of a reactionThe overall order of an elementary step directly corresponds to its molecularity. Both steps in thisexample are second order because they are each bimolecular. Furthermore, the rate law can bedetermined directly from the number of each type of molecule in an elementary step. For example, therate law for step 1 israte = k[NO2]?The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2israte = k[NO3]'[C0]! = k[NO3][CO]because the reaction involves only one molecule of each reactant the exponents are omitted.Analyzing a new reactionConsider the following elementary steps that make up the mechanism of a certain reaction:1. 2X→Y+ Z2. Y + 2L→M+Z What is the rate law for step 1 of this reaction?Express your answer in standard MasteringChemistry notation. For example, if the rate lawis k[A][C]° type k* [A] * [C]^3.• View Available Hint(s)Rate =

In an elementary reaction ,moleculaity becomes the order of the reaction Rate is directly…

Answered: What is the rate law for step 1 of this…

What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]% type k* [A] * [C]^3. View Available Hint(s)

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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For the standard Michaelis-Menten (MM) model (See image)If the experimenter accidentally setups the reaction such that [S]0 is not much greater than [E]0, derive the initial velocity of product formation, V0.
Consider the reaction data. A-products T (K)& (s- 325 0.376 875 0.719 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. yi = X2 = Determine the rise, run, and slope of the line formed by these points. rise: run: slope: What is the activation energy of this reaction? J/mol Ea =
0 State what rate law you would expect from this mechanism (Rate = k[Acetone]"[H*]"[[₂]') • Compare the expected rate law from the mechanism to the rate law you got from the Method of Initial rates and the Method of Isolation. If they are different, suggest 1-2 valid, specific, experimental reasons why they might be different. (fast, equilibrium) CH3 ソース H3C ག་ CH3 + H* = H3C H3C H. + H (slow) CH3 H3C CH2 + ↳2 Т + HI
3. The following reaction: A' (a) + B (ag + C (an)→ G* (ae) +2 H ) AH = -250 kJ There are two proposed mechanism: Mechanism 1 A' () + B aa) AB' a) + D (a) Step 1 AB" (a) (fast) + E (a) + Hm → G' sae) + H ) + D² (n) Step 2 (slow) Step 3 E (agi+ C (a) (fast) Mechanism 2: Step 1 AB' (a) A' (an) + B (ag) AB' (a) + C ja) (fast) Step 2 + G' (a) + 2 H() (slow) The reactions was determined to have the following rate law: r= k[A'][B] a) Which of the two proposed mechanisms is valid? Explain. b) List any reaction intermediates: catalysts: c) What is a rate determining step? d) If the activation energy for the overall forward reaction is 150 kJ, sketch the potential energy diagram for the above reaction; showing the overall reaction, the reaction mechanism, labelling the AHu, AHy, Eapu, Eag, reaction intermediates, and activated complex. rvs fwd drvs/
Consider the following elementary reaction: (g) (g) Suppose we let stand for the rate constant of this reaction, and stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of in terms of , , and the equilibrium concentration of .
The reaction for the decomposition of ammonia into its elements is: 2 NH3 (g) → N2 (g) + 3 H2 (g) [N2] 0.0105 M If the concentrations at a certain time are: what will be the associated value of the reaction quotient (Q)? [NH3] = 0.505 M [H2] = 0.414 M, %3D %3D (A) (B) (C) (D) (E) 0.00148 0.00292 0.00861 0.0105 342
tab esc slock ||| = OKINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi.... Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) + O₂ (g). -NO₂(g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O5 (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. BE 1 Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Explanation Q A @ 2 Check W S X # 3 E 0 rate = k 14 D $ 4 rate constant > R F % 5 © Stv T MacBook Pro 6 G We Y & 7 H 0-0 U 00 Ⓒ2022 McGraw Hill LLC. All R You * 00 00 8 S a (
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(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast
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