2N₂O5(soln) 4NO₂(soln) + O₂(g)Time (s)020040060080010001.000.880.780.690.610.540.480.430.380.340.30• Determine the order of reaction, half-life and rate constantRate Law:[N₂O5] (mol/L)Hint: Integrated rate laws for zero, first and second order reactions are shown belowOrderFirstRate = K[A]In[A] -kr+ In[A]oIntegrated Rate Law:Plot Needed to Give a Straight Line:Relationship of Rate Constantto the Slope of Straight Line:Half-Life:ZeroRate = k[A] = -kr + [A]o[A] versus fSlope-k[A]2k1200140016001800200011/2 =In[A] versusSlope-k0.693k11/2SecondRate = K[A]²[A]= kr +ASlopekfyz[A]oversus /=K[A]

A question based on kinetics of reaction in solution that is to be accomplished,

2N₂O,(soln) Rate Law: [N₂O3] (mol/L) Integrated Rate Law: 1.00 0.88 0.78 0.69 0.61 0.54 0.48 0.43 0.38 0.34 0.30 • Determine the order of reaction, half-life and rate constant Hint: Integrated rate laws for zero, first and second order reactions are shown below Order First Rate = K[A] In[A] -kr + In[A] Plot Needed to Give a Straight Line: Relationship of Rate Constant to the Slope of Straight Line: Half-Life: 4NO₂(soln) + O₂(g) Time (s) 0 200 400 600 800 1000 1200 1400 1600 1800 2000 Zero Rate = k [A] = -kr + [A] [A] versus r Slope-k [A] 2k In[A] versus t Slope--k 0.693 11/2² Second Rate = K[A]² kr + 11/2 [A] versus / [A] Slope-k A[A]

2N₂O,(soln) Rate Law: [N₂O3] (mol/L) Integrated Rate Law: 1.00 0.88 0.78 0.69 0.61 0.54 0.48 0.43 0.38 0.34 0.30 • Determine the order of reaction, half-life and rate constant Hint: Integrated rate laws for zero, first and second order reactions are shown below Order First Rate = K[A] In[A] -kr + In[A] Plot Needed to Give a Straight Line: Relationship of Rate Constant to the Slope of Straight Line: Half-Life: 4NO₂(soln) + O₂(g) Time (s) 0 200 400 600 800 1000 1200 1400 1600 1800 2000 Zero Rate = k [A] = -kr + [A] [A] versus r Slope-k [A] 2k In[A] versus t Slope--k 0.693 11/2² Second Rate = K[A]² kr + 11/2 [A] versus / [A] Slope-k A[A]

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

How do you determine the overall order of the reaction?
Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO₂(g) [NO]i (M) [0₂]i (M) 0.030 0.030 0.060 A) Rate = 57 M-1s-1 [NO][0₂] B) Rate = 3.8 M-1/2-1[NO][0₂]¹/2 C) Rate = 3.1 x 105 M-³s-1 [NO]²[0₂]² D) Rate = 1.7 × 103 M-2s-1 [NO]²[0₂] E) Rate = 9.4 × 103 M-²s-1 [NO][0₂]² 0.0055 0.0110 0.0055 Initial Rate (M-1,-1) 8.55 × 10-3 1.71 × 10-2 3.42 × 10-2
Consider the following data showing the initial rate of a reaction (A→products) at several different concentrations of A. [A](M) Initial rate (M/s) 0.15 0.014 0.30 0.055 0.60 0.220 You may want to reference (Page) Section 14.3 while completing this problem.
Some measurements of the initial rate of a certain reaction are given in the table below. [H2] [12] initial rate of reaction 2.42M 1.68 M 0.0836M/s 2.42M 3.71 M 0.185 M/s 0.848 M 1.68 M 0.0293 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k☐ k = = 0 x10 ☐ □·□
Calculate the rate constant considering the following rate data obtained at 25oC for the following reaction.
n=1
5. A generic reaction between A and Bas the equation: ZA[aq) + B(s) AzB(aq) To determine the differential rate law, the following experiments were performed with different initial molar concentrations of each: Initial Rate, Experiment [A], M [B), M M/s 1 0.100 0.100 0.00143 2 0.200 0.100 0.00572 3 0.100 0.200 0.00286 a. What is the differential rate law of the reaction? What are the orders b. What is the rate constant with proper units? c. What is the integrated rate law describing the concentration of A at a point in time t for experiment 1? d. How much A is in the reaction solution of experiment 1 at t=2.00 seconds? e. What is the integrated rate law describing the concentration of B at a point in time t for experiment 1? f. How much B is in the reaction solution of experiment 1 at t=2.00 seconds?
A student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -4,257.15 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.
n
Consider the reaction and the information in the table provided. Calculate the average rate of formation of P2O5 between 20.0s and 40.0s. 2H3PO4 → P2O5 + 3H2O Time (s) 0.0 10.0 20.0 30.0 40.0 50.0 Conc P2O5 (M) 0 0.00120 0.00420 0.00600 0.00720 0.00780
A student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -3,378.84 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.
The reaction 2NO(g) + Cl2 (g) -----> 2NOCl (g) was studied at –10°C. The following results were obtained where Rate = - Delta [Cl2]/ delta t [NO]0 [Cl2]0 Initial Rate (mol/L) (mol/L) (mol/L·min) 0.11 0.11 0.24 0.11 0.22 0.48 0.22 0.22 1.92 a Question Content Area What is the rate law? ( Use k for the rate constant. ) Rate =