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Chapter 12: Q85E. (page 716)

Based on the diagrams in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?

Short Answer

Expert verified

Reactions (a) and (b) have the same rate.

Step by step solution

01

Definition of Catalyst, Activation Energy

Catalyst are substances which increases the rate of the reaction without getting used up by themselves while decreasing the activation energy of the reaction. Activation energy is the energy difference between the initial reagents and the transition state(it is the state where the energy is maximum on the reaction coordinate diagram).

02

Determination of Fastest and Slowest Rate 

  • Catalyst increases the rate of reaction.
  • Catalyst accelerates the rate of a reaction by decreasing the activation energy.
  • Catalysts may provide different reaction mechanisms involving extra steps in the reaction and lower the activation energy simultaneously increasing the reaction rate.
  • Catalyst is regenerated during the reaction.

As both reactions (a) and (b) have same activation energy, these two reactions have same rate. Thus, reactions both (a) and (b) have the same rate.

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Most popular questions from this chapter

Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.

For each of the following pairs of reaction diagrams, identify which of the pairs iscatalyzed:

In a transesterification reaction, a triglyceride reacts with an alcohol to form an ester and glycerol. Many students learn about the reaction between methanol (\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH}}\)) and ethyl acetate (\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{OCOC}}{{\bf{H}}_{\bf{3}}}\)) as a sample reaction before studying the chemical reactions that produce biodiesel:

\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH + C}}{{\bf{H}}_{\bf{3}}}{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{OCOC}}{{\bf{H}}_{\bf{3}}}{\bf{ - - - C}}{{\bf{H}}_{\bf{3}}}{\bf{OCOC}}{{\bf{H}}_{\bf{3}}}{\bf{ + C}}{{\bf{H}}_{\bf{3}}}{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{OH}}\).The rate law for the reaction between methanol and ethyl acetate is, under certain conditions, determined to be: rate =\(k\left( {{\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{OH }}} \right)\). What is the order of reaction with respect to methanol and ethyl acetate, and what is the overall order of reaction?

Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, for the reaction was measured at several different temperatures, and the data are shown here:

Temperature(K)

k(M-1s-1)

555

6.23*10-7

575

2.42*10-6

645

1.44*10-4

700

2.01*10-3

What is the value of the activation energy (in kJ/mol) for this reaction?

Tripling the concentration of a reactant increases the rate of a reaction nine-fold. With this knowledge, answer the following questions:

  1. What is the order of the reaction with respect to that reactant?
  2. Increasing the concentration of a reactant by a factor of four increases the rate of a reaction four-fold. What is the order of the reaction with respect to that reactant?
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