Consider the reaction A > B. The initial [A] is 0.10M. After 1.0 hour, 50% of A has reacted. a. Draw agraph of concentration vs. time for each of thecases below. i. The reaction is zero order in A. I. Thereaction is first order in A. b. Predict what theconcentration of A will be after 2.0 hours for eachcase in part a if the initial [A] were 0.050 M. Explainyour reasoning.

Approach to solving the question: Detailed explanation: Examples: Key references:

Answered: Consider the reaction A > B. The…

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

18. Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of 0.271 s-1. f you start with 0.051 M I2 at this temperature, how much will remain after 5.05 s assuming that the iodine atoms do not recombine to form I2? M
6. Experimental data are listed for the hypothetical reaction A + B- C + D Time (s) 10 20 30 40 50 [A], M 0.38 0.29 0.24 0.20 0.17 0.15 а. Plot these data: [A] versus time. b. Draw a tangent to the curve to find the instantaneous rate at 25 s. С. Find the average rate over a 10 – 40 s interval. d. Compare the instantaneous rate at 25 s with the average rate over the 30 s interval.
9
The rate law for the reaction A - P is rate = k[A]³. The first half-life of the reaction is 20 seconds, what is the time for the second half-life? (to guarantee some marks you can submit your calculations) Select one: O a. 40 seconds O b. 160 seconds O . 80 seconds O d. 10 seconds O e. 20 seconds
A particular reaction is proposed to be first order. What plot would support this conclusion? a. a linear plot of [reactant] versus time b. an exponential decay of [reactant] versus time c. a linear plot of ln [reactant] versus time d. an exponential decay of ln [reactant] versus time
5. A laboratory experiment was done for the reaction below and the following data was obtained: A→ Products a. Reaction order. Time (hours) Concentration of A, mg/L 0 1 Plot the data in Excel and determine the following: b. Reaction rate, k. 23468 135 119 104 88 73 41 10
The following data were obtained from a study of the decomposition of CHEM at 320 oC: t, seconds Concentration of CHEM, mole/L 0.00 2.32 400 1.72 800 1.30 Plot the data using the first- and second-order equations. What is the order for this reaction? a. second order b. first order
what is the answer?
Half-life of a reaction The order of the reaction, ? → products, is being determined through the half-life method. Two setups at the same temperatures but different starting concentrations of A were investigated. For the first run, the initial concentration of A was 0.78 M and the halflife was determined to be 45 minutes. In the second run, the initial concentration of A was 1.32 M. Determine the following : a. If the reaction is 1st order, what should be the half-life of the second run in minutes? b. If the reaction is 2nd order, what should be the half-life of the second run in minutes? c. If the reaction is 0th order, determine the concentration of A in the second run after 152.3 minutes.
14. The overall order of reaction for the elementary reaction A + 2B a. 0 b. 1 c. 2 d. 3 * > Cis 15. If the volume of a container for the above reaction (Problem 14) is suddenly reduced to ½ its original volume with the moles of A, B & C maintained constant, the rate will increase by a factor of a. 2 b. 4 c. 8 d. 16
The reaction between hydrogen and chlorine is as follows: Cl2(g) + H2(g) → 2HCl(g) Experiments show that this reaction is first order with respect to H2 and one-half order with respect to Cl2. What is the rate law? a. Rate = k [H2]1/2 [Cl2] b. Rate = k [Cl2] [H2]2 c. Rate = k [Cl2]1/2 [H2] d. Rate = k [Cl2]2 [H2]
Molecular iodine, I2 (g), dissociates into iodine atoms at 652 K, with a first order rate constant of 0.452 s-1. I2(g) -----> 2I a. What is the half life for this reaction? b. If you start with 0.35 M I2 at this temperature, how long will it take for the concentration of I2 to reach 0.12 M?

SEE MORE QUESTIONS

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