A. B. С 00 Please provider your answer below. 0₂ For a second order reaction, the initial concentration of the reactant is 0.2402 M, and the first half life is 12.64 minutes. M-¹ min¹ 00 What is value of the rate constant? Check answer + Check answer What is the molarity of the reactant at 29.73 minutes AFTER the first half-life? Please provider your answer below. 00 + H Please provider your answer below. 0₂ What is the molarity of the reactant after 3 half-lives (The half-life may NOT be constant!) from the beginning of the experiment? M + →> $ (0) A + $ (0) A $ (0) A

A. B. С 00 Please provider your answer below. 0₂ For a second order reaction, the initial concentration of the reactant is 0.2402 M, and the first half life is 12.64 minutes. M-¹ min¹ 00 What is value of the rate constant? Check answer + Check answer What is the molarity of the reactant at 29.73 minutes AFTER the first half-life? Please provider your answer below. 00 + H Please provider your answer below. 0₂ What is the molarity of the reactant after 3 half-lives (The half-life may NOT be constant!) from the beginning of the experiment? M + →> $ (0) A + $ (0) A $ (0) 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...

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Part B Consider the second-order reaction: 2HI(g)→H₂(g) + I₂(g) Use the simulation to find the initial concentration [HI], and the rate constant k for the reaction. What will be the concentration of HI after t = 5.44x10¹0 s ([HI]) for a reaction starting under the condition in the simulation? Express your answer in moles per liters to three significant figures. ► View Available Hint(s) for Part B for Part do for Part redo for Part B res@or Part B keyboard shortcuts for Part B help for Part B [HI] = 1.6810³ Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining mol L
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Use the figure provided below to graphically estimate the instantaneous rate of change in the concentration of N₂O5 at t = 150 min. (Ent [N₂ 05] (M) Submit Answer 3 2.5 2 1.5 1 0.5 0 0 M min¹ Try Another Version 50 100 Time (minutes) 2 item attempts remaining 150 200
Please solve using exact numbers and do not round prematurely, and use proper sig figs and units. Thanks!
Which one is rate determining step in iodine clock reaction and why is it different from stoichiometric equation?
Enabled: Exam 2 Be sure to answer all parts. Consider the reaction A+B Products From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. [A] (M) | [B] (M) Rate (M/s) A. 匚 1.50 1.50 2.50 01 x 07 Reaction 1.50 6.40 x 10 Proctorio is sharing your screen. Stop sharing < Prev 10 of 17
< 11:28 A) Zeroth What order of reaction has a linear curve when plotting concentration versus time? B) First C) Second Question 6 of 12 D) Third Submit E) All reaction orders have a linear curve when plotted Tap here or pull up for additional resources
1:18 Sun, 16 June bb. = University of South Australia Dashboard Course Outline Content Academic Integrity Assessment In Grades Ө SP2 2024 Chemistry 100 Dashboard > CHEM 1006 > Online Quizzes > Online quiz 4 Question 4 If the rate law for the reaction Correct Mark 1.00 out 2A + 3B → products of 1.00 Remove flag is first order in A and second order in B, then the rate law is rate = a. k[A][B] b. k[A][B]² c. K[A]²[B]² d. k[A][B] e. k[A]²[B] Extensions Resources Your answer is correct. The correct answer is: k[A][B]² Recordings 16 b *༢ དཱི51% 10 ? Yunseo Kwon = ||| о Sunday, 16 June 2024 1:18 am ACST ←
2:11 A) S-¹ B) M-¹s-¹ The units for the rate constant for a zero order reaction are C) M. s-¹ Question 5 of 15 D) M-²S-¹ 5GW Tap here or pull up for additional resources Submit
Proposed mechanism: 03 K₁ K-1 0 + 03 0₂ + O K2 Questions: 20₂ 2 03 3 02 (fast equilibrium) (much slower irrev. step) (net rxn, gas phase) Experimental Observations: • Double initial [03] ==> rate increases 4X • Add [0₂] initially ==> rate drops (1) What is the chemical flux eqn for the proposed mechanism in terms of +d[O₂]/dt? (2) What is the SSA eqn for [O]? (3) What is the derived rate law for this mechanism in terms of +d[0₂]/dt? (4) Based on the exptl observations and derived overall rate law, is the proposed mechanism a plausible one for this rxn?