3. The decomposition of N2O5 in the gas phase was studied at constant temperature,2N2O5 (g) → 4NO2 (g) + O2(g)The following results were collected:findnature)N2O5]0.1000Ln[N2O5]-2.302.652.99-3.69-4.38-5.08a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time andTime (s)10g.(LN)0.07070.0500500.02501000.01252000.00625300400Ln[N2O5] versus time. Determine the value of k. Which graph didyou use?graph*b. On your graph of [N2O5] versus time, highlight the times it takes for each halving ofthe reactant concentration. What is the half-life? Using this half-life calculate k.design experiments to find the activation energy, KInetics Problems Laboratory1. Using the following chemical equation and data:A=Second order reactantB-first order reactantSimilarto3A + B+ 2C →D+2EExperimentnotesExамpleInitial [A]1.0 x 1021.0 x 1022.0 x 1022.0 x 102Initial [B]4.0 x 1038.0 x 1038.0 x 10-38.0 x 10-3Initial [C]2.0 x 1022.0 x 1022.0 x 10,21.0 x 1021Initial Rate25 mM/s310 mM/s *40 mM/s *40 mM/s4Determine the rate equation.b. Calculate the specific rate constant (k).Determine the initial rate of reaction if the initial concentrations of A, B, C are3 x 102 M, 5 x 10-3 M, 5 x 103M, respectively, for the reaction.a.с.a.) Rate= [A]²CB]'b.) K= rateCAJ C6]' = 5 m/s(10x (0-2) 2 (4.0x10-3)'=2M!5-1%3DC.)2. The reaction between bromate ions and bromide ions in acidic aqueous solution is givenby the following equation:BrO3 (aq) + 5Br (aq) +6H* (aq) → 3B12 (1) + 3H2O (1)

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Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.60E

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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
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.
Consider the following reaction: CH3X+YCH3Y+X At 25C, the following two experiments were run, yielding the following data: Experiment 1: [Y]0 = 3.0 M [CH3X] (mol/L) Time(h) 7.08 103 1.0 4.52 103 1.5 2.23 103 2.3 4.76 104 4.0 8.44 l05 5.7 2.75 l05 7.0 Experiment 2: [Y]0 = 4.5 M [CH3X] (mol/L) Time(h) 4.50 103 0 1.70 103 1.0 4.19 104 2.5 1.11 104 4.0 2.81 l05 5.5 Experiments also were run at 85C. The value of the rate constant at 85C was found to be 7.88 108 (with the time in units of hours), where [CH3X]0 = 1.0 102 M and [Y]0 = 3.0 M. a. Determine the rate law and the value of k for this reaction at 25C. b. Determine the half-life at 85C. c. Determine Ea for the reaction. d. Given that the C8X bond energy is known to be about 325 kJ/mol, suggest a mechanism that explains the results in parts a and c.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
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Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
For the following reaction C(s)+2H2(g)CH4(g) K=0.26 at 1000C (3 significant figures). What is the equilibrium constant at 750C (3 significant figures)?
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.
Enter the general form of the rate law for the following process. Represent the order as n, n', and so forth. Complete the equation using brackets, [], to represent concentration. 2Cu(g) + O2(g) → 2CuO(g) Please check to see if this was sent already. I do not see it in the pending questions
Consider the reaction between bromine and chlorine gases to form bromochloride: Br2(g)+Cl2(g)⇌2BrCl(g), Kc=1.11×10−4Br2(g)+Cl2(g)⇌2BrCl(g), Kc=1.11×10−4 at 150K150K A reaction vessel contains 0.20M Br20.20M Br2, 0.35M0.35M Cl2Cl2, and 3.0×10−3M BrCl3.0×10−3M BrCl. Calculate the reaction quotient, QQ, and determine in which direction the reaction proceeds to reach equilibrium. View Available Hint(s) Consider the reaction between bromine and chlorine gases to form bromochloride: at A reaction vessel contains , , and . Calculate the reaction quotient, , and determine in which direction the reaction proceeds to reach equilibrium. a. 4.3×10–24.3×10–2, the reaction system proceeds to the left b. 1.1×10–41.1×10–4, the reaction system is at equilibrium c. 1.3×10−41.3×10−4, the reaction system proceeds to the left d. 1.3×10–41.3×10–4, the reaction system proceeds to the right
What are Pseudo unimolecular reactions? Explain with the help of a suitable example.
Consider this reaction:H,CO; (aq) - H,O (ag) + CO, (ag)At a certain temperature it obevs this rate awrate = (0.067 5 ") [H,CO,]Suppose a vessel contains H, CO; at a concentration of 0.870 M. Calculate how long it takes for the concentration of Hz CO, to decrease to 9.0% of its initialvalue. You may assume no other reaction is important.Round your answer to 2 significant digits.

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