A student obtained the following data for the gas phase decomposition of hydrogen peroxide at 400 °C. H₂O₂(g) H₂O(g) + 2 O₂(g) [H₂0₂], M seconds 0.134 0 6.70x10-2 14.2 3.35x10-² 42.7 (1) What is the half-life for the reaction starting at t=0 s? 1.68x10-² 99.2 S S What is the half-life for the reaction starting at t=14.2 s? Does the half-life increase, decrease or remain constant as the reaction proceeds?

A student obtained the following data for the gas phase decomposition of hydrogen peroxide at 400 °C. H₂O₂(g) H₂O(g) + 2 O₂(g) [H₂0₂], M seconds 0.134 0 6.70x10-2 14.2 3.35x10-² 42.7 (1) What is the half-life for the reaction starting at t=0 s? 1.68x10-² 99.2 S S What is the half-life for the reaction starting at t=14.2 s? Does the half-life increase, decrease or remain constant as the reaction proceeds?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.5: Temperature And Reaction Rate: The Arrhenius Equation

Problem 11.9E: The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the...

See similar textbooks

Similar questions

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.
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.
For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at 720. K. If the initial pressure of A is 536 torr at 295C, how long will it take for the pressure of A to decrease to 268 torr?
The decomposition of NH3 to N2 and H2 was studied on two surfaces: Surface Ea (kJ/mol) W 163 Os 197 Without a catalyst, the activation energy is 335 kJ/mol. a. Which surface is the better heterogeneous catalyst for the decomposition of NH3? Why? b. How many times faster is the reaction at 298 K on the W surface compared with the reaction with no catalyst present? Assume that the frequency factor A is the same for each reaction. c. The decomposition reaction on the two surfaces obeys a rate law of the form Rate=k[NH3][H2] How can you explain the inverse dependence of the rate on the H2 concentration?
The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
For a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.
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.