23. A reaction proceeds by a series of elementary steps as shown below. The activation energy and heat of reaction are shown for each step. Step No. Elementary Step Activation Energy Enthalpy of Reaction 1 АВ — А + 72B, 12 kJ 35 kJ C + B, → CB, 2.5 kJ -29 kJ 3 АС > А + С 7.5 kJ 21 kJ a) What is the overall equation for this reaction? Show your work. b) What is the heat of reaction for the overall equation? Show your work. c) Which step is the rate determining step and why?

23. A reaction proceeds by a series of elementary steps as shown below. The activation energy and heat of reaction are shown for each step. Step No. Elementary Step Activation Energy Enthalpy of Reaction 1 АВ — А + 72B, 12 kJ 35 kJ C + B, → CB, 2.5 kJ -29 kJ 3 АС > А + С 7.5 kJ 21 kJ a) What is the overall equation for this reaction? Show your work. b) What is the heat of reaction for the overall equation? Show your work. c) Which step is the rate determining step and why?

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 11.109PAE

See similar textbooks

Similar questions

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?
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
Compare the functions of homogeneous and heterogeneous catalysts.
Why awe elementary reactions involving three or more reactants very uncommon?
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
Explain why half-lives are not normally used to describe reactions other than first order.
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g)CO2(g)+H2(g) The rate of reaction is monitored by measuring the total pressure in the reaction container. Time (s) Pressure (torr) 0 220 50 324 100 379 150 408 200 423 250 431 300 435 Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (HINT: Find the partial pressure of formic acid using Dalton's law of partial pressure and the reaction stoichiometry to find PHCOOH at each time.)
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
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.