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Chapter 12: Q77E. (page 712)

Account for the increase in reaction rate brought about by a catalyst.

Short Answer

Expert verified

Catalysts increases the rate of the reaction by decreasing the activation energy, by involving another reaction mechanism by allowing the reaction to attain equilibrium faster.

Step by step solution

01

Definition of catalyst

Catalyst are substances which increases the rate of the reaction without getting used up by themselves while decreasing the activation energy of the reaction.

02

Increase in the Reaction rate bought by a catalyst

  • Catalysts increase the rate of reaction by decreasing the activation energy. Example: Catalytic hydrogenation (alkene hydrogenation).
  • Many reactions occur at thermodynamically favourable conditions, but in the presence of catalyst, reactions occur at reasonable rate.
  • As the catalyst decrease the activation energy, it increases both forward and reverse reaction and makes reaction to attain equilibrium very fast.
  • The below graph represents the catalyzed and uncatalyzed alkene hydrogenation.

Thus, catalysts increase the rate of the reaction without taking part in the reaction and allows the reaction to attain equilibrium quickly.

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Most popular questions from this chapter

The rate constant for the first-order decomposition at 45 °C of dinitrogen pentoxide, N2O5, dissolved in chloroform, \({\bf{CHC}}{{\bf{l}}_3}\), is 6.2 × 10−4 min−1.

\({\bf{2}}{{\bf{N}}_{\bf{2}}}{{\bf{O}}_{\bf{5}}} \to {\bf{4N}}{{\bf{O}}_{\bf{2}}}{\bf{ + }}{{\bf{O}}_{\bf{2}}}\)

What is the rate of the reaction when \({{\bf{N}}_{\bf{2}}}{{\bf{O}}_{\bf{5}}}{\bf{\; = 0}}{\bf{.40 M}}\)

In terms of collision theory, to which of the following is the rate of a chemical reaction proportional?

(a) the change in free energy per second

(b) the change in temperature per second

(c) the number of collisions per second

(d) the number of product molecules

How do the rate of a reaction and its rate constant differ?

Use the PhET Reactions & Rates interactive simulation to simulate a system. On the “Single collision” tab of the simulation applet, enable the “Energy view” by clicking the “+” icon. Select the first A + BC⟶AB + C reaction (A is yellow, B is purple, and C is navy blue). Using the “straight shot” default option, try launching the A atom with varying amounts of energy. What changes when the Total Energy line at launch is below the transition state of the Potential Energy line? Why? What happens when it is above the transition state? Why?

A study of the rate of the reaction represented as 2A⟶ B gave the following data:

  1. Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s.
  2. Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus (A). What are the units of this rate?
  3. Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.
See all solutions

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