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Ch.14 - Chemical Kinetics
All textbooksTro 4th EditionCh.14 - Chemical KineticsProblem 83
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Chapter 14, Problem 83

How long will it take for 90% of the CH3CN to convert to CH3NC at 500 °C given the tabulated data: Time (h) [CH3CN] (M) 0.0 1.000, 5.0 0.794, 10.0 0.631, 15.0 0.501, 20.0 0.398, 25.0 0.316?

Verified step by step guidance
1
<Determine the order of the reaction by analyzing the concentration data over time.>
<Use the integrated rate law for the determined order to find the rate constant, k.>
<Calculate the concentration of CH3CN when 90% has converted to CH3NC, which is 10% of the initial concentration.>
<Use the integrated rate law with the calculated concentration and rate constant to solve for the time required for 90% conversion.>
<Verify the calculated time by checking if it aligns with the trend observed in the tabulated data.>
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Related Practice
Textbook Question

Suppose that the reaction A¡products is exothermic and has an activation barrier of 75 kJ/mol. Sketch an energy diagram showing the energy of the reaction as a function of the progress of the reaction. Draw a second energy curve showing the effect of a catalyst.

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Open Question
Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25 °C? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical.)
Textbook Question

The activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ/mol. If an enzyme increases the rate of the hydrolysis reaction by a factor of 1 million, how much lower must the activation barrier be when sucrose is in the active site of the enzyme? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical and a temperature of 25 °C.)

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Textbook Question

The tabulated data were collected for this reaction at 500 °C: CH3CN(g) → CH3NC( g) a. Determine the order of the reaction and the value of the rate constant at this temperature.

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Textbook Question

The tabulated data were collected for this reaction at 500 °C: CH3CN(g) → CH3NC( g) b. What is the half-life for this reaction (at the initial concentration)?

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Open Question
What is the half-life for this reaction at the initial concentration?