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Ch.14 - Chemical Kinetics

Chapter 14, Problem 95a

Consider this energy diagram:

a. How many elementary steps are involved in this reaction?

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Welcome back everyone in this example, we need to identify the number of elementary steps of the mechanism that is represented by the energy diagram below. When it comes to identifying elementary steps for a reaction, we should recall that for each peak in our diagram that would represent an elementary step. And so we want to count each peak in our graph below. So we would see that we have our first peak here, so this is our first elementary step, we have a second peak here, and then a third peak here. And so we would say that therefore we have a total of three peaks Which will correspond to three elementary steps for our reaction. And so our final answer is going to be three elementary steps are represented in the diagram. So I hope that everything I explained was clear. If you have any questions, leave them down below and I will see everyone in the next practice video.
Related Practice
Textbook Question

Consider the reaction: 2 O3(g) → 3 O2( g) The rate law for this reaction is: Rate = k [O3]2 [O2] Suppose that a 1.0-L reaction vessel initially contains 1.0 mol of O3 and 1.0 mol of O2. What fraction of the O3 will have reacted when the rate falls to one-half of its initial value?

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Textbook Question

Dinitrogen pentoxide decomposes in the gas phase to form nitrogen dioxide and oxygen gas. The reaction is first order in dinitrogen pentoxide and has a half-life of 2.81 h at 25 °C. If a 1.5-L reaction vessel initially contains 745 torr of N2O5 at 25 °C, what partial pressure of O2 is present in the vessel after 215 minutes?

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Textbook Question

Iodine atoms combine to form I2 in liquid hexane solvent with a rate constant of 1.5⨉1010 L/mols. The reaction is second order in I. Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial [I] concentration of 0.0100 M. How long will it take for 95% of the newly created iodine atoms to recombine to form I2?

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Textbook Question

Consider this energy diagram:

d. Is the overall reaction endothermic or exothermic?

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Textbook Question

Consider the reaction in which HCl adds across the double bond of ethene: HCl + H2C=CH2 → H3C-CH2Cl The following mechanism, with the accompanying energy diagram, has been suggested for this reaction:

Step 1 HCl + H2C=CH2 → H3C=CH2+ + Cl-

Step 2 H3C=CH2+ + Cl- → H3C-CH2Cl

a. Based on the energy diagram, determine which step is rate limiting.

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Textbook Question

Consider the reaction in which HCl adds across the double bond of ethene: HCl + H2C=CH2 → H3C-CH2Cl The following mechanism, with the accompanying energy diagram, has been suggested for this reaction:

Step 1 HCl + H2C=CH2 → H3C=CH2+ + Cl-

Step 2 H3C=CH2+ + Cl- → H3C-CH2Cl

b. What is the expected order of the reaction based on the proposed mechanism?

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