Hydrogen peroxide (H;O;) decomposes into water and awygen.H,O;(a9) + H0(1) + 1/2 0,(a)Ordinarily, this reaction proceeds rather slowty, but in the presence of some iodide ions (I ), the decomposition is much faster. The decomposition in the peesence of indide was studied at 20 C, and the data were plotted in various ways. Lise the graphs helow to answer the questions that follow.M (mol/L)1/M (L/mal)0.-0.50.1406--0.55-044-1.5-0.33-0242-Tlme (s)Tlme (s)Tlme (s)1003000001000001003000a What is the order of reaction for the decomposition of hydrogen peroxide?O zero-oderO first-onderOsecond-cederb. Find the numerical value of the rate constant at 20'C, including the correct units. (Enter an uneounded value.)k=C. Cbeain an estimate of the initial rate of reaction in the experiment that penduced the graphs (i.e, the rate at = 0 in the graphs) (Enter an unrounded value.)rate =Jmol - L

a.The reaction is first order as graph of lnM verses time graph is straight line. b. rate constant…

Hydrogen peroxide (H;O2) decamposes into water and owygen. H,O;(ag) + H0(1) + 1/2 0,(a) Ordinarily, this reaction proceeds rather slowty. hut in the presence of some iodide ions (I , the decompositicn is mach faster. The decomposition in the peesence of indide was studied at 20 C, and the data were plotted in various ways. Lise the graphs helow to answer the questions that follow. M (mol/L) 1/M (L/mol) 0. -0.5 014 1. 0.6 0.5 5- 04 -1.5- 03 3- 024 2- Tlme (s) Tlme (s) Tlme (s) 100 300 600 100 290 500 000 600 a What is the order of reaction for the decomposition of hydrogen peroxide? O zero-onder O first-order O second-ceder b. Find the numerical value of the rate constant at 20C, including the correct units. (Enter an uneounded value.) k= c. Ckeain an estimate of the initial rate of reaction in the experiment that penduced the graphs (i.e, the rate at e= 0 in the graphs) (Enter an unrounded value.) rate = Jmol · L

Hydrogen peroxide (H;O2) decamposes into water and owygen. H,O;(ag) + H0(1) + 1/2 0,(a) Ordinarily, this reaction proceeds rather slowty. hut in the presence of some iodide ions (I , the decompositicn is mach faster. The decomposition in the peesence of indide was studied at 20 C, and the data were plotted in various ways. Lise the graphs helow to answer the questions that follow. M (mol/L) 1/M (L/mol) 0. -0.5 014 1. 0.6 0.5 5- 04 -1.5- 03 3- 024 2- Tlme (s) Tlme (s) Tlme (s) 100 300 600 100 290 500 000 600 a What is the order of reaction for the decomposition of hydrogen peroxide? O zero-onder O first-order O second-ceder b. Find the numerical value of the rate constant at 20C, including the correct units. (Enter an uneounded value.) k= c. Ckeain an estimate of the initial rate of reaction in the experiment that penduced the graphs (i.e, the rate at e= 0 in the graphs) (Enter an unrounded value.) rate = Jmol · L

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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For the gas phase decomposition of hydrogen peroxide at 400 C 2 H2O2-->2 H20 + O2 the average rate of disappearance of H2O2 over the time period fromt-Os to t 61 sis found to be 5.07 10 we The average rate of formation of O2 over the same time period is Ms
17. If one defines the rate of the reaction 30 CH3OH +B10H14 0 10 B(OCH3)3 + 22 H2 as -A[B10 H14] At Rate = then the rate is also correctly expressed by 1 A[CH3 OH] At 1 ΔΒ(0CH> )s] At 1 A[H;] (a) Rate = 30 (b) Rate = 10 (c) Rate = 22 At (d) none of these. (e) all of these.
The reaction aA → products gives a plot of [A] vs time (in seconds) which is astraight line with a slope of -4.50×10–3. Assuming [A]0 = 0.200 M, how manyseconds are required for the reaction to reach 60.0% completion.
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The following initial rate data are for the reaction of UO,* with hydrogen ion in aqueous solution: 2 UO,* + 4 H*u* + UO,2* + 2 H,0 Experiment [UO,l,, M |[н"), м Initial Rate, M s! 2.43x10-3 9.70x10 3 4.85x10-3 1.94x10-2 4.36x10-3 8.72x103 0.886 0.886 4.36x10-3 1.77 14 8.72x103 1.77 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 = From these data, the rate constant is м?1
4
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