Order and rate law of a reactionThe overall order of an elementary step directiy 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 numberof each type of molecule in an elementary step. For example, the rate law for step 1 israte = k[NO2The exponent "2" is used because the reaction involves two NO, molecules. The rate law for step 2 israte = k[NO3]" [co]' = k[NO=][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. 3XE+F2. E+ M+F+NPart AWhat is the overall reaction?Express your answer as a chemical equation.• View Available Hint(s)Templates Symbols undo redo teset keyboard shortcuts HeipDA chemical reaction does not occur for this question. Part BWhich species is a reaction intermediate?> View Available Hint(s)O EO FO MNSubmitPart CWhat 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]*[CJ^3.> View Available Hint(s)Rate=SubmitPart DWhat is the rate law for step 2 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)Rate =

Answered: Image /qna-images/answer/8b22fcd1-3c98-4411-abd3-a3f0e545ab14.jpg

Answered: Part A What is the overall reaction?…

Part A What is the overall reaction? Express your answer as a chemical equation. • View Available Hint(s) Templates Symbols undo redo teset keyboard shortcuts Heip

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...

See similar textbooks

Similar questions

Please answer I really need help
Please show all work!
MISSED THIS? Watch KCV: The Rate of a Chemical Reaction, IWE: Expressing Reaction Rates; Read Section 15.2. You can click on the Review link to access the section in your eText. Consider the reaction Cl₂ (g) + 3F2 (g) → 2ClF3 (g), A[Cl₂]/At = -0.062 M/s. Part A Determine A[F2]/At. Express your answer to two significant figures and include the appropriate units. ► View Available Hint(s) A[F₂]/At= 0.186 Submit μA Part B Previous Answers M S X Incorrect; Try Again; 5 attempts remaining ? Determine A[CIF3]/At. Express your answer to two significant figures and include the appropriate units. ► View Available Hint(s)
Answer all the parts please
19. The initial rate of reaction between Substance A and Substance B was measured at a series of concentrations of each reactant with the following results. Solve for the rate law expression of this reaction. Note: Include all rough notes, show all calculations, follow the rules of significant figures, and box your final answer. ( A + B → AB Trial Number Trial #1 Trial #2 Trial #3 [A] 0.10 M 0.30 M 0.30 M [B] 0.10 M 0.10 M 0.20 M Initial rate 5.0 X 104 1.5 X 103 6.0 X 103 (mol/L·s)
Using the data and/or graph shown below, determine the rate of the reaction A-> products over the time period from t -80 s to ty s. Express your answer in decimal form in units of M/s, but do not add the units to your answer, just give the number. Concentration of A (moles/L) vs Time 0.900 1.000 0.900 10 0.621 0.800 20 0.474 0.700 30 0.383 0.600 40 0.321 0.500 50 0.277 0.400 60 0.243 0.300 70 0.217 0.200 80 0.196 0.100 90 0.178 0.000 0. 20 40 60 80 100 120 100 0.164 time(s)
Please help me