Rampless Unimeleculo gras a Eimaon - Bee 1) A chemical reaction proceeds with the proposed reaction mechanism below; Step Kinetics Assignment SCH4U0 E (kJ/mol) 754H +175 25-AH Ne) +Oze) → N;0 +O«). +50 1 N20 +Oe → NOe + NO«) -150+AH +25 3. NO +O + N0e) a) Draw the potential energy diagram for this reaction below. 300 250 P. Е. 200 (k J/ 150 mo 1) 100 Nte +0, 2(g) 50 b) What is the overall reaction? Nzg) + 2 0xg -> c) Which step is the rate determining step? Explain why. step 2 because it has the highest activation energy. d) What would be the rate law for this reaction? K= [ e) Explain what would happen to the rate if the concentration of Ne doubled. f) Use a dotted line to show what would happen if a catalyst was added to the reaction. g) Identify the spot on the graph that represents the transition state for reaction 2. Lono produced and

Rampless Unimeleculo gras a Eimaon - Bee 1) A chemical reaction proceeds with the proposed reaction mechanism below; Step Kinetics Assignment SCH4U0 E (kJ/mol) 754H +175 25-AH Ne) +Oze) → N;0 +O«). +50 1 N20 +Oe → NOe + NO«) -150+AH +25 3. NO +O + N0e) a) Draw the potential energy diagram for this reaction below. 300 250 P. Е. 200 (k J/ 150 mo 1) 100 Nte +0, 2(g) 50 b) What is the overall reaction? Nzg) + 2 0xg -> c) Which step is the rate determining step? Explain why. step 2 because it has the highest activation energy. d) What would be the rate law for this reaction? K= [ e) Explain what would happen to the rate if the concentration of Ne doubled. f) Use a dotted line to show what would happen if a catalyst was added to the reaction. g) Identify the spot on the graph that represents the transition state for reaction 2. Lono produced and

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 Constanta, @gic US UIC Taic an O IncicacUGHT. rate = If the rate constant for this reaction at 1000 K is 6.0 x 104 M-²s¹, what is the reaction rate when [NO] 2.30×10-2 M and [H₂] = 1.30×10-2 M? Express your answer using two significant figures. 10 ΑΣΦ L Xª Xb a √x Vx rate= [H₂] [NO]² f t C IXI 0 ? X-10" 8 M/s
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every way " D ← A Z → с L Remaining Time: 36 minutes, 39 seconds, Question Completion Status: Question 2 Moving to the next question prevents changes to this answer. HHH/ 1 1/1 1/ https://bbhosted.cuny.edu/webapps/assessment/take/take.jsp?course assessment_id=... A T O combination O combustion O single-replacement O double-replacement O decomposition 509 Rain coming S x What type of reaction is the reaction shown below (the classic experiment which led to the law of conservation of mass)? 2HgO(s) 2Hg(1) + O₂(g) Moving to the next question prevents changes to this answer. E OL 12 A R N T DEC OVE B a H N - de U M 8 K 9 O ✔ alt B 9 ? ( 1 C ctri 63 MC 3 pause MC + Question 2 of 15 6.667 points ♡ Save Answer Question 2 of 15 > backspace 8:34 A 10/24/20 enter ↑ shift CORE
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Consider chemical reaction:- X +2Y+ az )XY2Z2 It is faund that mng the [X] quadaup the [2] oubles the hate -) doubling the Cx7 has no effect on the sate doulbl les the late dneponb Cx] (- what is -the fate seaction 9 2 Pse dict the reactants for the Tate determ inA step. what is the molecularlty of the rate-deter step. minir 2) Predict a Complete mechanism Ahat meets the aiteria por this reaction Indicate which is neccessory the slow step the intermediates •J need these answer within 30 min. Thank Xou, Pleaze Consider g reguest my
For the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C 2 N₂O5 4 NO2 + O2 the average rate of disappearance of N₂O5 over the time period from t = 0 min to t = 159 min is found to be 5.79x10-4 M min¹¹. The average rate of formation of O₂ over the same time period is M min-¹.
nder [reactant), Treactant]," rate, rate; What is the reaction order with respect to A? (A), mol/L (B), mol/L rate, mol/(L-min) Trial 1 0.931 0.549 0.0781 Trial 2 1.86 0.549 0.0781 Trial 3 0.931 1.10 0.312 Trial 4 0.466 0.829 0.178 Rate = k(A]ordera B]arderb 2
5 Br-(aq) + BrO3-(aq) + 6 H+(aq)--> 3 Br2(aq) + 3 H2O(l); (a) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant A disappearance/decomposition.)
For the reaction: BrO3-(aq) + 5Br (aq) + 8H*(aq) → 3Br2(/) + H201) The initial rate of the reaction has been measured at the reactant concentration show: Trial [BrO;] (mol/L) 1 [H'] [Br ] Initial rat (mol/L) (mol/L) (mol/L-s) 0.10 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 The value for k will be: A L/mol.s Ouestion 13 (1 23
The following experimental data were obtained for the reaction of NH, and NO2 in acidic solution. NH, + (aq) + NO2 (aq)N2 (g) +2 H20(e) NH, ] (mol L) INO, | (mol L-1) Rate = A[N2]/At (mol L-s) %3D 0.0048 0.054 7.78 x 10-8 0.027 3.89 x 10-8 0.0048 0.0254 0.108 8.24 x 10-7 0.0130 0.108 4.20 x 10-7 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant = Submit Answer Try Another Verslon 9 item attempts remaining