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,

Answered: Image /qna-images/answer/4a0c5893-d80d-4735-ac46-d1b4b21e9bd1.jpg

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: find nature) N2O5] 0.1000 Ln[N2O5] -2.30 -2.65 -2.99 -3.69 -4.38 -5.08 Time (s) 0.0707 0. (LN) 0.0500 50 0.0250 100 200 0.0125 300 0.00625 400 a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and Ln[N2O5] versus time. Determine the value of k. Which graph did Yaph b. On your graph of [N20s] versus time, highlight the times it takes for each halving of you use? the reactant concentration. What is the half-life? Using this half-life calculate k.

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: find nature) N2O5] 0.1000 Ln[N2O5] -2.30 -2.65 -2.99 -3.69 -4.38 -5.08 Time (s) 0.0707 0. (LN) 0.0500 50 0.0250 100 200 0.0125 300 0.00625 400 a. Complete the table. Using the data and graph paper, plot the [N2O5] versus time and Ln[N2O5] versus time. Determine the value of k. Which graph did Yaph b. On your graph of [N20s] versus time, highlight the times it takes for each halving of you use? the reactant concentration. What is the half-life? Using this half-life calculate k.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.99PAE: Substances that poison a catalyst pose a major concern for many engineering designs, including those...

See similar textbooks

Similar questions

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?
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)?
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
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
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.
Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.
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.
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
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.
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.
The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?