QUESTION 31What are the units of k in the following rate law?Rate = k[X] [Y]M²○ MsMO M-1 s-1QUESTION 32What data should be plotted to show that experimental concentration data fits a first-order reaction?O In[reactant] vs. timeO In(k) vs. EaO [reactant] vs. timeO In(k) vs. 1/T1/[reactant] vs. time

Answered: QUESTION 31 What are the units of k in…

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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Q1
O Macmillan Learning Using the data in the table, determine the rate constant of the reaction and select the appropriate units. k = A + 2B C + D Trial [A] (M) [B] (M) Rate (M/s) 1 0.250 0.320 0.0152 2 0.250 0.640 0.0152 3 0.500 0.320 0.0608 Units
The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g)+CO(g)--->CO2(g)+NO(g) The following data were collected for the above reaction Experiment No [CO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0*10-4 1.6*10-2 1.7*10-7 2 5.0*10-4 3.2*10-2 1.7*10-7 3 1.5*10-3 3.2*10-2 1.5*10-6 Determine the order of the reaction with respect to each reactant.
Consider the generic reaction below. A + B --> C + D Given the following data and graph, determine the rate law for the reaction. Trial 1 [A] 0.10 M [B] 0.10 M Absorbance (A 1.55 1.50 1.45 1.40. 0 Rate = K[A]¹[B]⁰ Rate = K[A] [B]¹ Rate = K[A]²[B]O Rate = K[A]⁰[B]² Trail 2 0.20 M 0.10 M 0.5 Trial 1 Trial 2 1.0 Time (s) Trial 3 0.10 M 0.14 M Trial 3 1.5 2.0
consider the rate data at a certain temp for the reaction 2NO(g) + 2H2(g) --> N2(g) + 2H2O(g) determine the order of the reaction with respect to nitrogen monoxide
O Macmillan Learning Using the data in the table, calculate the rate constant of this reaction. k = A + B C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.330 0.240 0.330 0.624 0.528 0.240 Rate (M/s) 0.0234 0.158 0.0374
3
13:32 Mon Mar 8 * 33% O + : 1. a. For a reaction with the stoichiometry, 2 A = P, write an expression that relates the rate of disappearance of A to the rate of appearance of P. b. For a reaction with the stoichiometry, A + 2 B = 3 P, write an expression that relates the rate of disappearance of A to the rate of disappearance of B and another expression that relates the rate of disappearance of A to the rate of appearance of P. 2. What is the function of the Na,S,O, solution in the first part of this experiment? 3. What are the functions of solutions KCl and K,SO4 in this experiment? 1 4. What is the purpose of using the CUSO4 solution in this experiment?
The following set of data was obtained for the reaction below. What is the rate of reaction when [NO] = 0.00105M and [H2] = 0.0083M? . 2H2(8) + 2NO(8) 2H2O(g) + N2(8) Exp [NO], M [H2]. M Rate, M/s 1 0.0060 0.0010 0.180 2 0.0060 0.0020 0.360 3 0.0010 0.0060 0.030 4 0.0020 0.0060 0.120 5.0 x 106 Ms-1 43.5 Ms-1 -1 0.046 Ms 1.3 x 10-4 Ms-1
Calculate the concentration [A] for a reaction A Product after 7.00 min, knowing that the initial concentration [A]o is 2.4 M, and the rate constant is 3.2x10-3 M-1sec-1. Edit Format Table 12pt v Paragraph v BIU T?v : hp 732006020610 f3 米 fo f9 @
Question 7 of 8 Submit A reaction has a rate law of Rate = (1.25 M-1s-1)[A][B]. What is the rate of the reaction %3D if [A] = 0.301 M and [B] = 0.280 %3D %3D M? |M/s 1 4 5 6 C 7 8 9. +/- x 100
A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [#] |H, Initial rate of reaction x10 1.23 M 1.86 M 3 4.00 x 10 Mls | M/s 1.23 M 0.309 M 0.716 M O Mis Mls 3.20 м do Ar

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