For a reaction in which A and B forms C, the following data were obtained from the experiment: [A],mol/L [B], mol/l Rate of formation of C „mol/L-s 7 x10-4 2.8 x10-3 1.4 x10-3 0.30 0.15 0.60 0.30 0.30 0.30 What is the numerical value of the rate constant, k? Select one: O a. 0.018 L/mol-s O b. 0.017 L/mol-s O c. 0.016L/mol-s d. 0.012 L/mol-s

For a reaction in which A and B forms C, the following data were obtained from the experiment: [A],mol/L [B], mol/l Rate of formation of C „mol/L-s 7 x10-4 2.8 x10-3 1.4 x10-3 0.30 0.15 0.60 0.30 0.30 0.30 What is the numerical value of the rate constant, k? Select one: O a. 0.018 L/mol-s O b. 0.017 L/mol-s O c. 0.016L/mol-s d. 0.012 L/mol-s

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 30E: The reaction 2I-(aq)+S2O82-(aq)I2(aq)+2SO42-(aq) was studied at 25C. The following results were...

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.
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.
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.
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
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.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
At low temperatures, the rate law for the reaction CO(g)+NO2(g)CO2(g)+NO(g)is as follows: rate=(constant)[ NO2 ]2. Which of the following mechanisms is consistent with the rate law? (a) CO+NO2CO2+NO(b) 2NO2N2O4(fast) N2O4+2CO2CO2+2NO(slow) (c) 2NO2NO3+NO(slow) NO3+CONO2+CO2(fast) (d) 2NO22NO+O2(slow) O2+2CO2CO2(fast)
Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
For a reaction involving the decomposition of Y, the following data are obtained: (a) Determine the order of the reaction. (b) Write the rate expression for the decomposition of Y. (c) Calculate k for the experiment above.