KMnO4 (aq) + H₂O2 (aq) → MnO2 (aq) + KOH (aq) + H₂O (1) + O2(g) r = AC02/At The initial rate of reaction was monitored by measuring the moles of oxygen produced per second and the following kinetic data collected. Trial [KMnO.] (mol/L) [H.O.] (mol/L) 1 2 3 4 5 6 0.001 0.002 0.003 0.004 0.004 0.004 a) Determine the rate law equation for the reaction. b) What is the overall order of this reaction? 0.004 0.004 0.004 0.001 0.002 0.003 Rate (mol/s) 0.003 0.012 0.027 0.002 0.016 0.054 c) By what factor would the reaction rate increase if both [KMnO.] and [H.O.] were tripled at the same time?

KMnO4 (aq) + H₂O2 (aq) → MnO2 (aq) + KOH (aq) + H₂O (1) + O2(g) r = AC02/At The initial rate of reaction was monitored by measuring the moles of oxygen produced per second and the following kinetic data collected. Trial [KMnO.] (mol/L) [H.O.] (mol/L) 1 2 3 4 5 6 0.001 0.002 0.003 0.004 0.004 0.004 a) Determine the rate law equation for the reaction. b) What is the overall order of this reaction? 0.004 0.004 0.004 0.001 0.002 0.003 Rate (mol/s) 0.003 0.012 0.027 0.002 0.016 0.054 c) By what factor would the reaction rate increase if both [KMnO.] and [H.O.] were tripled at the same time?

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

Given the attached data for the reaction below, determine the rate law and rate constant for the reaction. Predict the rate for experiment #4 in the data. 2ICl(g) + H2(g) -> I2(g) + 2HCl(g)
Be sure to answer all parts. The bromination of acetone is acid-catalyzed: H* CH,COCH, + Br; CH,COCH,Br +H + Br catalyst The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H ions at a certain temperature: Rate of ICH,COCH, Brz (M) Disappearance of Br (M/s) (M) (M) (1) 0.650 0.0650 0.0650 5.91 x 105 (2) 0.650 0.130 0.0650 5.91 x 10 5 (3) 0.650 0.0650 0.130 1.18 x 10 (4) 0.865 0.0650 0.260 3.14 x 10 (5) 0.865 0.0650 0.0650 7.86 x 105 (a) What is the rate law for the reaction? O rate-k[CH,COCH,(Br3l(H'] rate=k[CH,COCH,lIBr2|[H*) O rate=k[CH,COCH,J[BrH"] O rate-k{CH3COCH,J[Br2|[H? rate=k(CH,COCH,l[Br,l[H
Hey, what would the answer to this be :) \
Labflow - Course: U... M Inbox (2,487) The following initial rate data are for the reaction of ICI with hydrogen: 21C1+ H₂ → I₂+ 2HCl 1 2 Experiment [IC]o, M [H₂lo, M Initial Rate, M s-1 0.397 0.202 0.0296 0.794 0.202 0.0593 0.397 0.404 0.119 0.794 0.404 0.237 3 4 Rate = 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. k = Submit Answer Pro-Connect H [Review Topics] [References] Use the References to access important values if needed for this question. M-2.s 1 Q Retry Entire Group 9 more group attempts remaining File Explorer O Previous Next Save and Exit 3:37 9/19/20
:$:):$$:$:$:$/$
For the hypothetical reaction A + 2B 3C, the rate of appearance of C given by (A[C]/At) may also be expressed as O A[C]/At = -(2/3) A[B]/At O A[C]/At = -(3/2) A[B]/At O A[C]/At = -(1/2) A[A]/At %3D O A[C]/At = A[A]/At
Worksheet Rate and React
Which one is rate determining step in iodine clock reaction and why is it different from stoichiometric equation?
only D E F G
A+B → Products Run 1 2 3 [A]o (M) 1 1 2 [B] (M) 1 2 1 Initial Rate (M/sec) 1 2 4 Rate = k [A]² [B]. What is k (don't forget the units) = [k]?
Consider this initial rate data at a certain temperature in the table for the reaction OH (aq) OCI (aq) + I (aq) OI (aq) + Cl(aq) Determine the rate law. rate k [OC] (1) Answer Bank (1-1² [OH Trial 1 2 3 4 [I Jo [OCI ]o (M) [OH lo (M) (M) 0.00171 0.00171 0.510 0.00171 0.00299 0.510 0.00279 0.00171 0.643 0.00171 0.00299 0.826 [OCI"] [OH-] Initial rates (M/s) 0.000359 0.000629 0.000465 0.000388
Question 30 of 39 Submit The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.205 M. What is the value of k for this reaction? M/min 1 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources