The initial rates method can be used to determine the rate law for a reaction. Using the data for the reaction shown below,what is the rate law for the reaction?A+B CTrial [A] (1) [B](mol)A[A] molmolAt Ls10.0750.0750.135020.0750.0900.194430.0900.0750.1350•Report your value of k with two significant figures.Provide your answer below:rate=

Step 1: Step 2: Step 3: Step 4:

Answered: The initial rates method can be used to…

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

Use the following data to calculate the reaction rate law and the rate law constant for the system. ??(?)+?2(?)→???2(?) Trial Run [NO] (mol/L) [H2] (mol/L) Initial Rate (mol/L∙s) 1 0.001 0.004 0.002 2 0.002 0.004 0.008 3 . 0.003 0.004 0.018 4 0.004 0.001 0.008 5 0.004 0.002 0.016 6 . 0.004 0.003 0.024 a) rate = k[NO][H2]2, where k = 7 L2/mol2∙s b) rate = k[NO]2[H2], where k = 5.0x105 L2/mol2∙s c) rate = k[NO][H2], where k = 5.0x105 L2/mol∙s d) rate = k[NO]2[H2]3, where k = 3.0x10-7 L/mol2∙s
Determine the rate law and calculate the rate constant for this reaction: 2 NO (g) + Br₂(1)→2 NOBr (g) Initial [Br₂]/M Expt. 1 2 3 Initial [NO]/M 0.10 0.20 0.20 0.10 0.10 0.30 Initial rate/M.s-¹ 1.30 x 10-³ 5.20 x 10-³ 1.56 x 10-²
4. Given: A +B O C Rate ( M sec ') 4.0X 10 -5 4.0 X 105 16 X 10-5 [] 0.1 [B] 0.1 0.1 0.2 0.2 0.1 Determine the rate law. Calculate the rate constant. Determine the rate when [A] = 0.05 and [B] = 0.10
D
◇ KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 1.36M 1.21M 0.744 M/s 1.36M 0.393 M 1.44M 1.21M 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 0.0785 M/s 0.788 M/s 0 x10 ロ･ロ X 1/5
Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) [CH3CI] / mol L-1 Initial Rate / mol L-1 s-1 Trial [Cl2] / mol L-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the order of the reaction with respect to Cl2?
1. At elevated temperatures, nitrous oxide decomposes according to the equation2N2O(g)⟶2N2(g)+O2(g) Time (min) 0 60 90 300 600 [N2O] 0.250 0.228 0.216 0.128 0.0630 Given the following data, determine whether the reaction is zeroth, first, or second order. a) first b) second c) zeroth
g.
Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [H₂] [] initial rate of reaction 0.336M 2.08M 0.338 M/s 1.12M 2.08 M 1.13M/s. 0.336M 2.39M 0.388 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=& = 0 k= Contenti 0. 00 0° 0.0 X

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS