Fast pls i will give u thumsup fast MISSED THIS? Read Section 15.4 (Pages 642-650); WatchKCV 15.4.The data below show the concentration of N₂O5 versus timefor the following reaction:N2O5 (g) → NO3(g) + NO₂(g)Time (s) [N₂O5] (M)01.000250.8220.6770.5570.4580.3770.3100.2550.2105075100125150175200straight line, so the reaction must be first order in N₂O5.Part BDetermine the value of the rate constant.Express the rate constant to three significant figuresk=IVE ΑΣΦSubmitPart CPredict concentration of N₂O5 at 290 s.[N₂O5] =SubmitRequest AnswerProvido FoodbookDA[Π ΑΣΦRequest Answer?8-1?M

Given N2O5 (g) -----> NO3 (g) + NO2 (g) And data of time and concentration of N2O5

The data below show the concentration of N₂O5 versus time or the following reaction: N2O5 (g) → NO3(g) + NO₂(g) Time (s) [N₂O5] (M) 0 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210 Part B Determine the value of the rate constant. Express the rate constant to three significant figures k= [5] ΑΣΦ Submit Part C Predict the concentration of N₂O5 at 290 s. [N₂O5] = Request Answer Submit 15| ΑΣΦ Request Answer ? 8-1 ? M

The data below show the concentration of N₂O5 versus time or the following reaction: N2O5 (g) → NO3(g) + NO₂(g) Time (s) [N₂O5] (M) 0 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210 Part B Determine the value of the rate constant. Express the rate constant to three significant figures k= [5] ΑΣΦ Submit Part C Predict the concentration of N₂O5 at 290 s. [N₂O5] = Request Answer Submit 15| ΑΣΦ Request Answer ? 8-1 ? M

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 11.104PAE

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.
The reaction for the Haber process, the industrial production of ammonia, is N2(g)+3H2(g)2NH3(g) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 ×10-5 molL-1s-1. At what rate is nitrogen consumed? At what rate is hydrogen consumed?
The annual production of HNO3 in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel. (a) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)2NO2(g) (C) 3NO2(g)+H2O(l)2HNO3(aq)+NO(g) The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in O2, what is the rate of formation of NO2 when the oxygen concentration is 0.50 M and the nitric oxide concentration is 0.75 M? The rate constant for the reaction is 5.8106 L2/mol2/s.
Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?
Experiments during a recent summer on a number of fireflies (small beetles, Lampyridaes photinus) showed that the average interval between flashes of individual insects was 16.3 s at 21.0C and 13.0 sat 27.8C. a. What is the apparent activation energy of the reaction that controls the flashing? b. What would be the average interval between flashes of an individual firefly at 30.0C? c. Compare the observed intervals and the one you calculated in part b to the rule of thumb that the Celsius temperature is 54 minus twice the interval between flashes.
Based on the diagrams in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
Chlorine dioxide oxidizes iodide ion in aqueous solution to iodine; chlorine dioxide is reduced to chlorite ion. 2ClO2(aq)+2I(aq)2ClO2(aq)+I2(aq) The order of the reaction with respect to ClO2 was determined by starting with a large excess of I, so that its concentration was essentially constant. Then Rate=k[ClO2]m[I]n=k[ClO2]m where k= k[I]n. Determine the order with respect to ClO2 and the rate constant k by plotting the following data assuming first- and then second-order kinetics. [Data from H. Fukutomi and G. Gordon, J. Am. Chem. Soc., 89, 1362 (1967).] Time (s) [ClO2] (mol/L) 0.00 4.77 104 1.00 4.31 104 2.00 3.91 104 3.00 3.53 104 5.00 2.89 104 10.00 1.76 104 30.00 2.4 105 50.00 3.2 106
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?
The rate of the reaction O(g)+NO2(g)NO(g)+O2(g) was studied at a certain temperature. a. In one experiment, NO2 was in large excess, at a concentration of 1.0 1013 molecules/cm3 with the following data collected: Time(s) [O](atoms/cm3) 0 5.0 109 1.0 102 1.9 109 2.0 102 6.8 108 3.0 102 2.5 108 What is the order of the reaction with respect to oxygen atoms? b. The reaction is known to be first order with respect to NO2 Determine the overall rate law and the value of the rate constant.