Consider the following data for the reaction: A + B → C+D[B] (M)[D] (M)0.02000.0500.02000.0500.02000.2000.04000.050[A] (M)0.01000.02000.01000.0100The rate law is given byOk [A]² [B] [D]-1Ok [A]² [B]-¹ [D]¹/2Ok [A] [B]1/2 [D]-1/2Ok [A]-¹ [B] [D]¹/2Ok [A]-¹ [B] [D]-1/2Onone of the aboveThe rate constant k is equal to02.5 x 10³01.83601.4 x 10404.0 x 105The correct units for the rate constant areOM3/2 min-1OM¹/2 min-1Omin-1OM-1/2 min-1OM-¹ min-1Initial rate (M min-¹)15.9331.867.9722.53

Answered: Image /qna-images/answer/23649ecc-b290-4109-addf-268a7b040d3c.jpg

Consider the following data for the reaction: A+B → C+D [A] (M) [B] (M) 0.0100 0.0200 0.0200 0.0100 0.0100 The rate law is given by Ok [A]² [B] [D]-¹ Ok [A]² [B]-¹ [D]¹/2 Ok [A] [B]1/2 [D]-1/2 Ok [A] ¹ [B] [D]¹/2 Ok [A]-¹ [B] [D]-1/2 Onone of the above 0.0200 0.0200 0.0400 104 [D] (M) 0.050 0.050 0.200 0.050 The rate constant k is equal to 02.5 x 10³ 01.8 036 01.4 x 04.0 x 105 The correct units for the rate constant are OM³/2 min-1 OM¹/2 min-1 Omin-1 OM-1/2 min-1 OM-¹ min-1 Initial rate (M min-¹) 15.93 31.86 7.97 22.53

Consider the following data for the reaction: A+B → C+D [A] (M) [B] (M) 0.0100 0.0200 0.0200 0.0100 0.0100 The rate law is given by Ok [A]² [B] [D]-¹ Ok [A]² [B]-¹ [D]¹/2 Ok [A] [B]1/2 [D]-1/2 Ok [A] ¹ [B] [D]¹/2 Ok [A]-¹ [B] [D]-1/2 Onone of the above 0.0200 0.0200 0.0400 104 [D] (M) 0.050 0.050 0.200 0.050 The rate constant k is equal to 02.5 x 10³ 01.8 036 01.4 x 04.0 x 105 The correct units for the rate constant are OM³/2 min-1 OM¹/2 min-1 Omin-1 OM-1/2 min-1 OM-¹ min-1 Initial rate (M min-¹) 15.93 31.86 7.97 22.53

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

Consider the following chemical equation: Overall Reaction: A B2 + BC - AB + C + B2 The proposed mechanism is as follows: BC – B+ C (slow) A B2 + B = AB+ B2 (fast) What is the rate law? Rate = k[B C] O Rate = k[A B,][B] Rate = k[C] O Rate = k[B][C] Rate k[A B2][B C) Rate = k[A B][B,] Rate = k(A B2]
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
It was found that for the reaction 2 A + B → 3 C the rate law is Rate = k[A][B] · %3D At the initial concentrations [A]o = 0.100 M and [B]o = 0.200 M the initial rate is 0.0500 M/s. %3D What would be the initial rate if the initial concentrations were [A]o = 0.500 M and [B]o = 0.0750 M? 0.0352 M/s 0.0937 M/s O 0.0711 M/s 0.00533 M/s O 0.469 M/s
A reaction has a rate law of Rate = (1.25 M⁻¹s⁻¹)[A][B]. What is the rate of the reaction if [A] = 0.313 M and [B] = 0.280 M?
Which of the following is true for the rate law r= k[A]M[B]"? O A) The order of each species must be determined by experiment. B) Both m and n are restricted to positive integers. C) Both m and n can be obtained from the stoichiometry of the overall reaction. D) The overall order of the reaction is given by m x n.
A reaction has a rate law of Rate = (1.25 M⁻¹s⁻¹)[A][B]. What is the rate of the reaction if [A] = 0.327 M and [B] = 0.280 M?
A reaction has a rate law of Rate = (1.25 M⁻¹s⁻¹)[A][B]. What is the rate of the reaction if [A] = 0.713 M and [B] = 0.280 M?
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]
A+ B+ 2C - 2D+ 3E where the rate law is A[A] k[A][B]* Rate = - %3D At An experiment is carried out where [A], = 1.0 x 10-2 M, [B, = 6.0 M, and [C, = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. k%3= L mols 1 b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 17.0 seconds. Concentration= M d. Calculate the concentration of C after 17 seconds. Concentration=