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Chapter 12: Q84E. (page 716)

Based on the diagrams in Exercise 12.82, which of the reactions has the fastest rate? Which has the slowest rate?

Short Answer

Expert verified

Reaction (b) has the fastest rate. Reaction (a) has the slowest 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.
  • Catalyst is regenerated during the reaction.

Therefore, reaction (a) has higher activation energy compared to reaction (b). Hence, reaction (a) with higher activation energy has the slowest rate and reaction (b) with lower activation energy has the highest rate. Thus, reaction (a) has slowest rate and reaction (b) has the highest rate.

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Most popular questions from this chapter

How will each of the following affect the rate of the reaction:

\({\bf{CO}}\left( {\bf{g}} \right){\bf{ + \;N}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {{\bf{O}}_{\bf{2}}}{\bf{\;}}\left( {\bf{g}} \right){\bf{ + NO}}\left( {\bf{g}} \right)\) if the rate law for the reaction is rate = \({\bf{k(NO}}{}_{\bf{2}}{\bf{)(CO)}}\)?

  1. Increasing the pressure of \({\bf{NO}}{}_{\bf{2}}\) from 0.1 atm to 0.3 atm
  2. Increasing the concentration of CO from 0.02 M to 0.06 M.

Pure ozone decomposes slowly to oxygen,\({\bf{2}}{{\bf{O}}_{\bf{3}}}{\bf{(g)}} \to {\bf{3}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\). Use the data provided in a graphical method and determine the order and rate constant of the reaction.

Time(hr)

0

2.0x103

7.6x 104

1.00x104

1.23x104

1.43x104

1.70x104

(O3) (M)

1.0x10-5

4.98x10-6

2.07x10-6

1.66x10-6

1.39x10-6

1.22x10-6

1.05x10-6

Describe how graphical methods can be used to determine the activation energy of a reaction from a series of data that includes the rate of reaction at varying temperatures.

Doubling the concentration of a reactant increases the rate of a reaction four times. With this knowledge, answer the following questions:

  1. What is the order of the reaction with respect to that reactant?
  2. Tripling the concentration of a different reactant increases the rate of a reaction three times. What is the order of the reaction with respect to that reactant?

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?
See all solutions

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