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Ch.14 - Chemical Kinetics
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All textbooksTro 4th EditionCh.14 - Chemical KineticsProblem 97a

Chapter 14, Problem 97a

The desorption (leaving of the surface) of a single molecular layer of n-butane from a single crystal of aluminum oxide is found to be first order with a rate constant of 0.128/s at 150 K. a. What is the half-life of the desorption reaction?-

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Hey everyone in this example we have the hydraulics sis of the anticancer drugs CISplatin. It occurs with first order kinetics, with the following rate constant at 310.15 kelvin. And we need to determine the half life of the reaction. So we should recall that are half life for a first order reaction is going to equal the natural log of two, divided by our rate constant. So what we should have is that our half life of our hydraulic sis reaction is going to equal the Ln of two, divided by our rate constant, given in the prompt as 5.33 times 10 to the negative third power. And sorry, so times 10 to the negative third power in verse minutes. So in our calculators we want to find the value of this quotient on the right hand side here. And what we would get is that our half life is equal to a value of 130 minutes. And for our final answer this would be the half life of our hydraulic sis reaction of CISplatin. So I hope that everything I explained was clear. If you have any questions, please leave them down below. And I will see everyone in the next practice video
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Consider this energy diagram:

d. Is the overall reaction endothermic or exothermic?

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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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Textbook Question

The desorption (leaving of the surface) of a single molecular layer of n-butane from a single crystal of aluminum oxide is found to be first order with a rate constant of 0.128/s at 150 K. b. If the surface is initially completely covered with n-butane at 150 K, how long will it take for 25% of the molecules to desorb (leave the surface)? For 50% to desorb?

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Textbook Question

The evaporation of a 120-nm film of n-pentane from a single crystal of aluminum oxide is zero order with a rate constant of 1.92⨉1013 molecules/cm2•s at 120 K. a. If the initial surface coverage is 8.9⨉1016 molecules/cm2, how long will it take for one-half of the film to evaporate?

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Textbook Question

The kinetics of this reaction were studied as a function of temperature. (The reaction is first order in each reactant and second order overall.) C2H5Br(aq) + OH- (aq)¡C2H5OH(l ) + Br - (aq) Temperature (°C) k (L,mol # s) 25 8.81 * 10- 5 35 0.000285 45 0.000854 55 0.00239 65 0.00633 b. Determine the rate constant at 15 °C.

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