Q2) Consider the following third order reaction: A→ product The following is the integrated rate law for the third order reaction: 21A1-² 11/2 = 1.5 K[A],² 2[A],² If the concentration of the reactant after 26.5 second of the experiment was found to 0.348 M and the rate constant for this reaction was found to be 1.5x10² M².S¹. a) Determine the initial concentration of the reactant.

Q2) Consider the following third order reaction: A→ product The following is the integrated rate law for the third order reaction: 21A1-² 11/2 = 1.5 K[A],² 2[A],² If the concentration of the reactant after 26.5 second of the experiment was found to 0.348 M and the rate constant for this reaction was found to be 1.5x10² M².S¹. a) Determine the initial concentration of the reactant.

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 reaction for chlorine reacting with chloroform, Cl2 (g) + CHCIl3 (g) HС (g) + СCla (g) a) based on the initial rate data provided (in the table below), determine the rate law for this reaction. b) The following is a proposed mechanism for this reaction. Cl2 (g) = 2 CI (g) CI (g) + CHCI: (g) → HCI (g) + CCl: (g) (slow) CCl: (g) + CI (g) > Сle (g) (fast equilibrium) (fast) Is this an acceptable mechanism based on the rate law you determined in part a? answer should be Yes/No to "is this an acceptable mechanism") Initial Rate [CI,] [CHCI3] 0.00253 | 0.2 0.3 A) Yes 0.00759 0.2 0.9 B) No 0.00506 0.8 0.3
The reaction N2O5- 2NO2 + 1/2 O2(g) is first order. The rate constant k is 6.2 x 10-4/min. A) What is the half life of this reaction in seconds and days? B) How long will it take for the concentration of N2O5 to decrease to 25% of it's original concentration?
18.) A generic reaction has the rate law rate = k[A]2[B]1. What is the value of the rate constant, k, if the rate = 0.517 M/s when the [A] = 0.413 M and [B] = 0.904 M? Do not include units. Your Answer:
The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figures
The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)
The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 2E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.58E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt
The reaction of IC1 with hydrogen 2IC1 + H₂ → I2 + 2HCl is first order in IC1 and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [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 =
The reaction: NO (g) + O3 (g) —> NO2 (g) + O2 (g) Is thought to be a second-order reaction with respect to O3. You start with [O3] = 0.250 M. After 125 s you find that the [O3] has dropped to 0.145 M. A) Assuming the reaction is second order, determine the value and units of the rate constant. B) Determine the half-life of the reaction. C) Calculate [O3] after 195 seconds.