Do not apply the calculations, based on the approximation of the stationary state, to make them perform correctly. Basta discard the 3 responses that you encounter that are obviously erroneous if you apply the formula to determine the speed of a reaction. For the decomposition reaction of N2O5(g): 2 N2O5(g) · 4 NO2(g) + O2(g), the following mechanism has been proposed: N2O5 -> NO2 + NO3_(K1) NO2 + NO3 →> N2O5 (k-1) → NO2 + NO3 → NO2 + O2 + NO (K2) NO + N2O5 → NO2 + NO2 + NO2 (K3) Give the expression for the acceptable rate. (A). d[N₂O] dt = -1 2k,k₂[N205] k₁+k₂ d[N₂O5] (B). dt =-k₁[N₂O₂] + k₁[NO2][NO3] - k₂[NO2]³ (C). d[N₂O] dt =-k₁[N₂O] + k₁[N205] - K3 [NO] [N205] (D). d[N2O5] =-k₁[NO] - K3[NO] [N₂05] dt

Do not apply the calculations, based on the approximation of the stationary state, to make them perform correctly. Basta discard the 3 responses that you encounter that are obviously erroneous if you apply the formula to determine the speed of a reaction. For the decomposition reaction of N2O5(g): 2 N2O5(g) · 4 NO2(g) + O2(g), the following mechanism has been proposed: N2O5 -> NO2 + NO3_(K1) NO2 + NO3 →> N2O5 (k-1) → NO2 + NO3 → NO2 + O2 + NO (K2) NO + N2O5 → NO2 + NO2 + NO2 (K3) Give the expression for the acceptable rate. (A). d[N₂O] dt = -1 2k,k₂[N205] k₁+k₂ d[N₂O5] (B). dt =-k₁[N₂O₂] + k₁[NO2][NO3] - k₂[NO2]³ (C). d[N₂O] dt =-k₁[N₂O] + k₁[N205] - K3 [NO] [N205] (D). d[N2O5] =-k₁[NO] - K3[NO] [N₂05] dt

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

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 25Q: Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine...

See similar textbooks

Similar questions

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)?
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.
Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?
Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.
5.12. True or false: If all the partial pressures of reactants and products drop by half, the value of Q drops by half. Give an example of a chemical reaction to support your answer.
The recycling of polymers represents only one industrial process that allows creating order in one location by creating greater disorder at some other location, often at a power plant. List three other industrial processes that must create disorder in the surroundings to generate the desired material.
The gaseous compound dinitrogen pentoxide (N₂O₅) decomposes in air to yield nitrogen dioxide gas (NO₂) andoxygen gas (O₂). If we can determine the rate of this decomposition, we can also determine the concentration ofdinitrogen pentoxide in a given sample at any point in time. This reaction is typically conducted in an apparatus such as the following, in which the water bath is used to control the temperature surrounding the dinitrogen pentoxide gas. In your analysis, you’ll examine data collected during the decomposition of 0.25 M dinitrogen pentoxide gas. Theconcentrations of dinitrogen pentoxide, nitrogen dioxide, and oxygen were measured at eight different time points at normal atmospheric pressure and a temperature of 45°C. 1. Write a balanced equation for this decomposition reaction, including phase notations.
Nitrogen dioxide reacts with carbon monoxide by the overall equation NO:(9) + CO(g) → NO(9) + CO2 (9) At a particular temperature, the reaction is second order in NO, and zero order in CO. The rate constant is 0.515 L/(mol - s). How much heat energy evolves per second initially from 7.25 Lof reaction mixture containing 2.40 x 102 M NO,? NO: (9) + NO(g) + co(g) -110.5 kJ/mol + CO2(9) -393.5 kJ/mol AH; = 33.10 kl/mol. 90.29 kJ/mol Assume the enthalpy change is constant with temperature. Energy = kJ/s
The presence of a catalyst provides a reaction pathway in which the activation energy of a reaction is reduced by 42.00 kJ mol-¹. Uncatalyzed: Catalyzed: Keat Kuncat A → B A B Ea Ea kcat kuncat = = Determine the factor by which the catalyzed reaction is faster than the uncatalyzed reaction at 294.0 K if all other factors are equal. 122.00 kJ mol-1 80.00 kJ mol-1 times faster Determine the factor by which the catalyzed reaction is faster than the uncatalyzed reaction at 360.0 K if all other factors are equal. times faster
Pentaerythritol tetranitrate (abbreviated PETN, chemical formula C5H8N4O12) is an explosive material with a structure that is very similar to nitroglycerin. It is one of the components of plastic explosives such as Semtex. The explosion of PETN can be represented by: C5H8N4O12(s)→2CO(g)+4H2O(g)+3CO2(g)+2N2(g) A plastic explosive charge is formed into a cylinder about 30 cm long and about 2 cm in diameter. It weighs about 246 grams and is 58.5% PETN by mass. What is the total number of moles of gas produced when this plastic explosive charge explodes? mol gas Sulfuric acid (H2SO4) reacts with sodium bicarbonate (NaHCO3) to produce sodium sulfate, carbon dioxide and water. If 1.45 L of 4.50 M H2SO4 is spilled and 1.00 kg NaHCO3 (MM=84.01 g/mol) is available to clean up the spill, is there enough sodium bicarbonate to neutralize the spilled sulfuric acid? No, and there is about 10% less NaHCO3than needed. Yes, and there is about 10% more NaHCO3than needed.…
Pentaerythritol tetranitrate (abbreviated PETN, chemical formula C5H8N4O12) is an explosive material with a structure that is very similar to nitroglycerin. It is one of the components of plastic explosives such as Semtex. The explosion of PETN can be represented by: C5H8N4O12(s)→2CO(g)+4H2O(g)+3CO2(g)+2N2(g) A plastic explosive charge is formed into a cylinder about 30 cm long and about 2 cm in diameter. It weighs about 276 grams and is 58.5% PETN by mass. What is the total number of moles of gas produced when this plastic explosive charge explodes?
Chlorine dioxide (ClO₂) is a disinfectant used in municipal water treatment plants. It dissolves in basic solution producing ClO3 and ClO₂": 2 CLO₂(g) + 2 OH (aq) → ClO3(aq) + ClO₂ (aq) + H₂O(l) › The following kinetic data were obtained at 298 K for the reaction. Experiment [CIO₂]0 (M) [OH-]o (M) Initial Rate (M/s) 1 0.060 0.030 0.0248 2 0.020 0.030 0.00827 3 0.020 0.090 0.0247 Determine the rate law by indicating the values of "x" and "y" in the general rate law below. Rate = K[ClO₂]X[OH-]Y X = 1 = 1 y = OB b. Calculate the rate constant for this reaction at 298 K. Sig. Figs. are important. M-1. S-1 Rate constant, k = 184.4