7.13.74 The following data were collected for the reactionbetween hydrogen and nitric oxide at 700°C:Experiment1232H₂(g) + 2NO(g) →→ 2H₂O(g) + N₂(8)curied out at 430°C[H₂]0.0100.00500.010[NO]0.0250.0250.0125Initial Rate (M/s)2.4 x 10-61.2 × 10-60.60 × 10-6(a) Determine the order of the reaction. (b) Calcu-late the rate constant. (c) Suggest a plausible mech-anism that is consistent with the rate law. (Hint:Assume that the oxygen atom is the intermediate.)

Rate of any specific reaction at a particular reacting species concentration is the equivalent rate…

7. 13.74 The following data were collected for the reaction between hydrogen and nitric oxide at 700°C: 2H₂(g) + 2NO(g) →→2H₂O(g) + N₂(g) Experiment 1 2 3 [H₂] 0.010 0.0050 0.010 [NO] 0.025 0.025 0.0125 Initial Rate (M/s) 2.4 x 10-6 1.2 x 10-6 0.60 × 10-6 (a) Determine the order of the reaction. (b) Calcu- late the rate constant. (c) Suggest a plausible mech- anism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate.)

7. 13.74 The following data were collected for the reaction between hydrogen and nitric oxide at 700°C: 2H₂(g) + 2NO(g) →→2H₂O(g) + N₂(g) Experiment 1 2 3 [H₂] 0.010 0.0050 0.010 [NO] 0.025 0.025 0.0125 Initial Rate (M/s) 2.4 x 10-6 1.2 x 10-6 0.60 × 10-6 (a) Determine the order of the reaction. (b) Calcu- late the rate constant. (c) Suggest a plausible mech- anism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate.)

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 11.42PAE: Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small...

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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?
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
(5) IV. Hydrogen and carbon monoxide react to give formaldehyde under certain conditions. H2(g) + CO(g) = HCHO(g) The mechanism proposed for this reaction is H2(g) = 2 H(g) H(g) + CO(g) H(g),+ HCO(g) → HCHO What rate law is derived from this mechanism? Step 1 Step 2 Step 3 fast HCO(g) slow > fast
4. 3) The data given in the table below is for the following reaction (run at 25°C): 2 NO + O, → 2 NO, 2(g) 2(g) Initial Concentration (M) Initial rate Experiment Mol/(L s) NO 02 0.0010 7 X 10-6 1 0.0010 0.0010 0.0020 14 X 10-6 0.0010 0.0030 21 X 106 0.0020 0.0030 84 X 10-6 0.0030 0.0030 189 X 10-6 1. Determine the orders of the reaction with respect to NO and O, (show all work): NO O2
1. HBr +O2 →HOOBF 2(g) (slow) 2. НООBr + HBr, (8) 2HOB" 2g) (fast) 3. 2{НОBr + HBr, T →H,O« +Br} (fast) (8) (g) 2(g) 4HB +0,→2H,O, +2Br%e - (3) Consider the above reaction mechanism. The rate-law equation from this reaction would be - K[HOB1]*[HBr] K[HBr]*[O,] = k[HOB1]² r = k[HBr]'[O,]' а. r = d. = b. e. impossible to tell from this information r = с.
Consider the gas-phase reaction of nitric oxide with hydrogen at 1280°C 2NO(g) + 2H2(g) →N2(g) + 2H20(g) Experiment [NO](M) 5.00 x 10-3 1.00 x 10-2 1.00 x 10-2 [H2](M) 2.00 x 10-3 2.00 x 10-3 4.00 x 10-3 Initial Rate (M/s) 1.25 x 10-5 5.00 x 10-5 1.00 x 104 Determine the a. the rate law b. overall reaction order C. the rate constant, k. 123
Activated complex 400 (b) 300 Products Potential Energy (a) 200 (c) 100 Reactants Reaction Pathway Activated complex 400 (b) 300 Products Potential Energy (a) 200 (c) 100 Reactants Reaction Pathway Alex thinks that the graph above represents an exothermic reaction and the AH = +400kJ and energy will be released in this reaction. Is Alex correct? If not, find his error and then correct it with explanation. %3D
(ii) At elevated temperatures, nitrogen dioxide decomposes to nitric oxide and molecular oxygen: 2NO2(g) – → 2NO(g) + O2(g) The change in concentration of NO2 with time at 300 °C is given below: t (s) 100 200 300 400 500 [NO2]/103 (mol dm-3) 8.0 5.6 4.3 3.5 2.9 2.5 By appropriate plotting of the data and use of this graph: (a) verify that this reaction is second order with respect to NO2; (b) determine the rate constant for this reaction.
The study of the kinetics of the decomposition reaction of N205 gas was carried out in a closed cylinder with a volume of 1 L. The reactions that occur are: 2N2O5 (g) → 4N02(g) + O2(e) The following is a curve of 1/N205 against the reaction time of decomposition of N205 gas at temperatures of 427K and 527K. y = 2,0923x - 3,75 R² = 0,9999 0,7708x + 146,96 R² = 0,9995 ¥=0,7708x + 146,96 R² = 0,9995 %3D Time (sekon) a. Determine the rate equation for the decomposition reaction of gas N205 b. Determine the value of the rate constant (k) for the reaction at both temperatures. Express in the correct units. 1/[N,Og] (L/mol)
33) For the reaction PC15 (g) PC13 (g) + Cl2 (g) Kc= 0.0454 at 261°C. If a vessel is filled with these gases such that the initial concentrations are [PC15]= 0.2 M, [PC13] = 0.20 M, and [Cl2]= 2.25 M, in which direction will a %3D reaction occur and why? A) toward reactants becauseQ=1.8 B) toward reactants becauseQ= 0.0454 C) toward products becauseQ = 2.8 D) it is at equilibrium because Q=1 E) toward products becauseQ = 0.56
Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³
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