Please and thank you ? The following data are for the decomposition of hydrogen peroxide in dilutesodium hydroxide at 20 °C.H,02(aq) → H,0(I) + ½ 0,(g)H20(1) + ½ 02[H,0, ], M9.50x10-22.4.75x10422.38x10 21.19×10 2.time, min7.3514.722.1Hint: It is not necessary to graph these data.(1)The half life observed for this reaction ismin .(2)Based on these data, the rate constant for thisorder reaction ismin -1.zerofirstsecond

The decomposition of the hydrogen peroxide and the required time is as follows: H2O2, M 9.50×10-2…

The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H,02(aq) → H20(I) + ½ 0,(g) [ H,02 ], M 9.50x10 2 4.75x10 2 7.35 2.38x10 2 1.19x10 2 time, min 14,7 22.1 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this order reaction is min 1. zero first secon

The following data are for the decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C. H,02(aq) → H20(I) + ½ 0,(g) [ H,02 ], M 9.50x10 2 4.75x10 2 7.35 2.38x10 2 1.19x10 2 time, min 14,7 22.1 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is min . (2) Based on these data, the rate constant for this order reaction is min 1. zero first secon

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 11.48PAE: 11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol...

See similar textbooks

Similar questions

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.
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.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
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
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?
11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
The decomposition of hydrogen iodide on finely divided gold at 150C is zero order with respect to HI. The rate defined below is constant at 1.20 104 mol/L s. 2HI(g)AuH2(g)+I2(g)Rate=[HI]t=k=1.20104mol/Ls a. If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. b. How long will it take for all of the 0.250 M HI to decompose?
11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN. Time, t (min) Partial Pressure of PAN (torr) 0.0 2.00 X 10~’ 10.0 1.61 X 10~} 20.0 1.30 X 10_J 30.0 1.04 X 10"’ 40.0 8.41 X 10-4 50.0 6.77 x 10-4 60.0 5.45 X 10-4
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
Consider the decomposition reaction 2X2Y+ZThe following graph shows the change in concentration with respect to time for the reaction. What does each of the curves labeled 1, 2, and 3 represent?
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. SO2Cl2(g)SO2(g)+Cl2(g)At a certain temperature, the half-life of SO2Cl2 is 7.5102 min. Consider a sealed flask with 122.0 g of SO2Cl2. (a) How long will it take to reduce the amount of SO2Cl2 in the sealed flask to 45.0 g? (b) If the decomposition is stopped after 29.0 h, what volume of Cl2 at 27C and 1.00 atm is produced?