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 =

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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...

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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)
Question 23 The rate law for a reaction is determined to be rate=k[AJIB}*[C]. If the reaction has an overall order of 9, what is the value of exponent for B? (the answer should be entered as a single digit number; do not enter units; examples include 0 and 1 and 2 and 3 and etc.) K Questa A Moving to another question will save this response. B88 . 43C & %23 4 5 6. 8 3 I o P Q E R T Y tab A S F G K caps lock V B alt alt control option command command option
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537 of 5 33. The decomposition of nitrosyl chloride was studied: 2NO(g) + Cl₂(g) 2NOCI(g) The following data were obtained where A[NOCI] Copyright 2018 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Rate = [NOCI], (molecules/cm³) 3.0 × 10¹6 2.0 × 10¹6 X 1.0 X 10¹6 4.0 × 10¹6 Initial Rate (molecules/cm³-s) 5.98 × 104 2.66 X 10* 6.64 × 10³ 1.06 × 10³ 0.060 a. Determine the rate law. b. Calculate a value for the rate constan and an average value for the rate con a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the value of the rate constant when concentra- tions are given in moles per liter. 0.030 34. The following data were obtained for the gas-phase decompo- sition of dinitrogen pentoxide, 2N₂O₂(g) → 4NO₂(g) + O₂(g) 36. The reaction 2NO(g) + was studied, and the follo [NO] (molecules/cm³) 1.00 X 10¹8 3.00 × 1018 2.50 X 10¹8 Ra [ (molec 1.00 1.00 2.50 What would be the in [NO] 6.21 x 10¹8 1018…
Core Chemistry Skill: Balancing a Chemical Equation 5 of 33 > to form four moles of the product, water. Part A Balance the chemical equation by indicating the number of each species in the appropriate blanks. For this exercise, indicate coefficients of 1 explicitly. Match the numbers in the left column to the appropriate blanks in the chemical equations on the right. Make certain the chemical equation is complete before submitting your answer. • View Available Hint(s) Reset Help 1 Fe (s) + H2O (1) → Fe3 04 (s) + 2 Н2 (9) 3 4 Submit Previous Answers
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)
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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)
9. In Part C, what observation allows you to detect the decomposition of hydrogen peroxide?
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