For the reaction 2 NO (g) +2 H2 at1100° C, the following data have been obtained. N2 (G) + 2 H,Og [NO] [H,] Rate = -A[NO]/ At ( mol/Ls) (mol/L) (mol/ L) 5.0 x 10 3 0.32 0.012 1.0 x 10 2 0.32 0.024 1.0 x 10 2 0.64 0.096 Derive a rate law for the reaction, and determine the value of the rate constant, O a Rate = k [N,[H2 Of Ob. Rate = k [No[H Oc Rate = k [NO][H,F O d. Rate = k [NO][H,] k = 23 L/ mol-s k = 23L/mol-s %3D k = 23 L2 mol2s 1 k = 23L /mol-s

For the reaction 2 NO (g) +2 H2 at1100° C, the following data have been obtained. N2 (G) + 2 H,Og [NO] [H,] Rate = -A[NO]/ At ( mol/Ls) (mol/L) (mol/ L) 5.0 x 10 3 0.32 0.012 1.0 x 10 2 0.32 0.024 1.0 x 10 2 0.64 0.096 Derive a rate law for the reaction, and determine the value of the rate constant, O a Rate = k [N,[H2 Of Ob. Rate = k [No[H Oc Rate = k [NO][H,F O d. Rate = k [NO][H,] k = 23 L/ mol-s k = 23L/mol-s %3D k = 23 L2 mol2s 1 k = 23L /mol-s

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 31E: The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI]...

See similar textbooks

Similar questions

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.
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3 (termolecular reactions are improbable but possible). If the first half-tife of the reaction is found to he 40. s, what is the time for the second half-life? Hint: Using your calculus knowledge, derive the integrated rate law from the differential rate law for a tennolecular reaction: Rate=d[A]dt=k[A]3
The hypothetical reaction X(g)+12Y(g)productsis first-order in X and second-order in Y. The rate of the reaction is 0.00389 mol/L min when [X] is 0.150 M and [Y] is 0.0800 M. (a) What is the value for k? (b) At what concentration of [Y] is the rate 0.00948 mol/L min and [X] is 0.0441 M? (c) At what concentration of [X] is the rate 0.0124 mol/L min and [ Y ]=2[ X ]?
Use the data provided in a graphical method to determine the order and rate constant of the following reaction: 2PQ+W Time (s) 9.0 13.0 18.0 22.0 25.0 [P] (M) 1.077103 1.068103 1.055103 1.046103 1.039103
The activation energy for the decomposition of cyclobutane (C4H8) to ethylene (C2H4) is 261 kJ/mol. If the system produces ethylene at the rate of 0.043 g/s at 500C, what is the rate if the temperature increases to 600C?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
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.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
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 first-order rate constant for the decomposition of a certain hormone in water at 25C is 3.42104day1. (a) If a 0.0200 M solution of the hormone is stored at 25C for two months, what will its concentration be at the end of that period? (b) How long will it take for the concentration of the solution to drop from 0.0200 M to 0.00350 M? (c) What is the half-life of the hormone?