SavedThe following mechanism has been suggested for the reaction:11H2O2 + 2H+ + 21-→ I2 + 2H2OH2O2 +I-HOI + OH-OH-+H+ → H2OHOI + H+ +I-→I2 + H2OSlowFast3 01:24:24FastIdentify the rate law that is consistent with this mechanism.Multiple ChoiceRate = k[H202]Rate = k[HOITH"IRate = k[OH"][H"]Rate = k[HOITOH]Rete = k(H2O21?H"7?

Answered: Image /qna-images/answer/a65f3904-101a-4be0-827c-aa8278504ea1.jpg

Saved The following mechanism has been suggested for the reaction: 11 H2O2 + 2H+ + 21-→ I2 + 2H2O H2O2 +I- HỘI + OH- OH-+H+ → H20 HOI + H* +I-→2 + H2O Slow Fast X 01:24:24 Fast Identify the rate law that is consistent with this mechanism. Multiple Choice Rate = k[H2O21] Rate = k[HOITH I Rate = k[OH][H"] Rate = k[HOIIOH] Rete = k(H202H7?

Saved The following mechanism has been suggested for the reaction: 11 H2O2 + 2H+ + 21-→ I2 + 2H2O H2O2 +I- HỘI + OH- OH-+H+ → H20 HOI + H* +I-→2 + H2O Slow Fast X 01:24:24 Fast Identify the rate law that is consistent with this mechanism. Multiple Choice Rate = k[H2O21] Rate = k[HOITH I Rate = k[OH][H"] Rate = k[HOIIOH] Rete = k(H202H7?

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

The following reaction is first order in respect to CH3OH and first order in respect to HCl. With this in mind, what is the rate constant for the reaction? Be sure you choose the answer with the right units. CH3OH(aq) + HCL(aq) ----> CH3CL(aq) + H2O(i) Reaction CH3OH conc. HCl conc. Initial Rate (M/s) 1 0.100 M 0.100 M 1.1 x 10-2
T[C] K [ cm³/mol-s] The rxn is a decomposition reaction of HI. 2HI → H₂ + 1₂ In this rxn, the ff data were gathered. 508 1.059x10-1 427 3.1x10-3 393 5.88x10-4 356 8.09x10-5 Solve for the complete rate eq. for this reaction [ i.e. r = f(T) f(C) ] 283 9.42x10-7
The rate constant for the second order reaction 2 NO2 - 2 NO + O2 is 0.24 M's. If a 1.38 M sample of NO2 reacts for 47.7 seconds, what concentration of NO2 wil remain? Report your answer to two decimal places. |Al = - kt +|Alo InJAl = - kt + InlAlo TAI = kt + TAlo
For the reaction 2NO + Cl2 ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above NO + Cl2 NOCl2 fast equilibriumNOCl2 + NO 2NOCl slow 2NO N2O2 fast equilibriumN2O2 + Cl2 2NOCl slow Cl2 2Cl slowCl + NO NOCl fast NO + Cl2 NOCl + Cl slowCl + NO NOCl fast
What are the correct units for the rate constant in a zeroth order overall reaction rate? O M-1s1 O Ms1 s1 O None of these are correct.
A particular reaction is found to be zero order. The reactant has an initial concentration of 1.52 M and a rate constant of 0.00740 M/s. Calculate the half life of this reactant in seconds. t1/2 =[A]i/2k
None
Please make sure that the answer that I get is correct thank you so much
Determine the rate order and rate constant for dinitrogen pentoxide. Time (minutes) [N2O5] 0 0.0165 10.0 0.0124 20.0 0.00930 30.0 0.00710 40.0 0.00530 50.0 0.00390 60.0 0.00290 Group of answer choices First-order, k = 0.0289 minute-1 First-order, k = 0.0126 M-1⋅minute-1 Second-order, k = 4.59 M-1⋅minute-1 Zero-order, k = 0.000200 M/minute Zero-order, k = 0.0148 M/minute Second-order, k = 30.8 M-1⋅minute-1
. At body temperature, the first-order rate constant is 1.87 x 103 min¹ for the elimination of the cancer chemotherapy agent, cisplatin, from the human body. How many hours will it take for 2.5 x 10-3 M of cisplatin to decrease its concentration to 1.0 x 10-³ M? ray mamuntive 20 mucaraman uantment પર ભરોસ www male de contest menaces yetamanas
mechanism 1 overall reaction is 2NO + Cl2 --> 2NOCl NO + Cl2 = NOCl2 fast equilibriumNOCl2 + NO---> 2NOCl slow rate law for mechanism 1 is rate=k[no2]^2[cl2] mechanism 2 Cl2 --> 2Cl slowCl + NO --> NOCl fast rate law for this mechansim 2 is rate=k[cl2] i noticed that when the mechanism has a fast reaction at equilibrium, the rate law includes reactants form both fast and slow, whereas when the reaction has fast reactions not at equilibrium, the rate law is only the reactants from the slow step (rate determining step) why is the rate law different when the fast reaction is at equilibrium vs when the mechansim has a fast reaction not at equilibrium?
The first-order reaction, SO2C12 → SO2 + Cl2, has a rate constant equal to 2.20 × 10-5 s-1 at 593 K. What percentage of the initial amount of SO2C12 will remain after 9.2 hours? 100% 99.9% 3.88% 48.3% 2.20%