Potential Energy (kJ)1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction.ΔΗ = - 950 kJAH = 575 kJAH = -825 kJ(i) Cl₂ (g) + Pt (s) → 2C) (g) + Pt (s)(ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s)(iii) Cl (g) + CICO (g) → CI₂CO (g)260024002200200018001600140012001000800a. Draw the potential energy diagram for the reaction. Label the data points for clarity.The potential energy of the reactants is 600 kJ6004002000-200-400-600-800Ea = 1550 kJEa = 2240 kJEa = 2350 kJReaction Progressb. What is the overall chemical equation?c. What is the overall change in enthalpy for the above chemical reaction? d. What is the overall amount of activation energy for the above chemical reaction?e. Which reaction intermediate would be considered a catalyst (if any) and why?f. If you were to add 2700kJ of energy to the reaction (e.g. 2700 kJ of heat or electricity), wouldyou be able to make the reaction reverse itself (i.e. have the products become reactants)?Justify your answer.g. If you were to added a positive catalyst to step (ii) what would the end result be? Explain yourprediction.h. Your friend is looking at your graph and states that she believes that step (ii) is the ratedetermining step. Do you agree with her? If you do not agree with her, what step would youpick as the RDS?

#(a):Given the reaction proceeds via 3 elementary steps. So there will be 3 peaks in the potential…

1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) Cl₂(g) + Pt (s) → 2C) (g) + Pt (s) Ea = 1550 kJ (ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s) Ea - 2240 kJ ΔΗ = = 950 kJ ΔΗ = 575 kJ ΔΗ = = 825 kJ (iii) Cl (g) + CICO (g) → CI,CO (g) Ea - 2350 kJ 2600 2400 2200 2000 a. Draw the potential energy diagram for the reaction. Label the data points for clarity. The potential energy of the reactants is 600 kJ 1800 1600 1400 1200 1000 800 600 400 200 0 -200 -400 -600 -800- Reaction Progress b. What is the overall chemical equation? c. What is the overall change in enthalpy for the above chemical reaction?

1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) Cl₂(g) + Pt (s) → 2C) (g) + Pt (s) Ea = 1550 kJ (ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s) Ea - 2240 kJ ΔΗ = = 950 kJ ΔΗ = 575 kJ ΔΗ = = 825 kJ (iii) Cl (g) + CICO (g) → CI,CO (g) Ea - 2350 kJ 2600 2400 2200 2000 a. Draw the potential energy diagram for the reaction. Label the data points for clarity. The potential energy of the reactants is 600 kJ 1800 1600 1400 1200 1000 800 600 400 200 0 -200 -400 -600 -800- Reaction Progress b. What is the overall chemical equation? c. What is the overall change in enthalpy for the above chemical reaction?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.68QE

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In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
Assuming that the mechanism for the hydrogenation of C2H4 given in Section 11-7 is correct, would you predict that the product of the reaction of C2H4. with D2 would be CH2DCH2D or CHD2CH3? How could the reaction of C2H4 with D2 be used to confirm the mechanism for the hydrogenation of C2H4 given in Section 11-7?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
Write a rate law for NO3(g) + O2(g) NO2(g) + O3(g) if measurements show the reaction is first order in nitrogen trioxide and second order in oxygen.
Nitrogen dioxide reacts with carbon monoxide by the overall equation NO2(g)+CO(g)NO(g)+CO2(g) At a particular temperature, the reaction is second order in NO2 and zero order in CO. The rate constant is 0.515 L/(mol s). How much heat energy evolves per second initially from 3.50 L of reaction mixture containing 0.0275 M NO2? See Appendix C for data. Assume the enthalpy change is constant with temperature.
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
11.44 A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 4.0 X 10_H s"' at 25°C. What is the half-life for the degradation of DDT in this experiment, in years?

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