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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

Thefollowingdatahave been determined for the reaction: \({{\bf{I}}^{\bf{ - }}}{\bf{ + OC}}{{\bf{l}}^{\bf{ - }}} \to {\bf{I}}{{\bf{O}}^{\bf{ - }}} + {\bf{C}}{{\bf{l}}^{\bf{ - }}}\)

1

2

3

\({{\bf{(}}{{\bf{I}}^{\bf{ - }}}{\bf{)}}_{{\bf{initial}}}}\)(M)

0.10

0.20

0.30

\({{\bf{(OC}}{{\bf{l}}^{\bf{ - }}}{\bf{)}}_{{\bf{initial}}}}\)(M)

0.050

0.050

0.010

Rate(mol/l/s)

\({\bf{3}}{\bf{.5*1}}{{\bf{0}}^{{\bf{ - 4}}}}\)

\({\bf{6}}.{\bf{2*1}}{{\bf{0}}^{{\bf{ - 4}}}}\)

\({\bf{1}}.{\bf{83*1}}{{\bf{0}}^{{\bf{ - 4}}}}\)

Determine the rate equation and the rate constant for this reaction.

Does the following data fit a second-order rate law?

Trial

Time(s)

(A) (M)

1

5

0.952

2

10

0.625

3

15

0.465

4

20

0.370

5

25

0.308

6

35

0.230

Ingeneral, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A + B鉄禖? Can we predict the effect if the reaction is known to be an elementary reaction?

Given the following reactions and the corresponding rate laws, in which of the reactions might the elementary reaction and the overall reaction be the same?\(\begin{aligned}{\rm{(a) C}}{{\rm{l}}_2}{\rm{ + CO }} \to {\rm{ C}}{{\rm{l}}_2}{\rm{CO}}\\{\rm{rate = }}k{{\rm{(C}}{{\rm{l}}_2}{\rm{)}}^{\frac{3}{2}}}{\rm{(CO)}}\\{\rm{(b) PC}}{{\rm{l}}_3}{\rm{ + C}}{{\rm{l}}_{\rm{2}}}{\rm{ }} \to {\rm{ PC}}{{\rm{l}}_{\rm{5}}}\\{\rm{rate = }}k{\rm{(PC}}{{\rm{l}}_{\rm{3}}}{\rm{) (C}}{{\rm{l}}_{\rm{2}}}{\rm{)}}\\{\rm{(c) 2NO + }}{{\rm{H}}_{\rm{2}}}{\rm{ }} \to {\rm{ }}{{\rm{N}}_{\rm{2}}}{\rm{ + }}{{\rm{H}}_{\rm{2}}}{\rm{O}}\\{\rm{rate = }}k{\rm{(NO)(}}{{\rm{H}}_{\rm{2}}}{\rm{)}}\\{\rm{(d) 2NO + }}{{\rm{O}}_{\rm{2}}}{\rm{ }} \to {\rm{ 2N}}{{\rm{O}}_{\rm{2}}}\\{\rm{rate = }}k{{\rm{(NO)}}^{\rm{2}}}{\rm{(}}{{\rm{O}}_{\rm{2}}}{\rm{)}}\\{\rm{(e) NO + }}{{\rm{O}}_{\rm{3}}}{\rm{ }} \to {\rm{ N}}{{\rm{O}}_{\rm{2}}}{\rm{ + }}{{\rm{O}}_{\rm{2}}}\\{\rm{rate = }}k{\rm{(NO)(}}{{\rm{O}}_{\rm{3}}}{\rm{)}}\end{aligned}\)

Iodine-131 is a radioactive isotope that is used to diagnose and treat some forms of thyroid cancer. Iodine-131 decays to xenon-131 according to the equation:I-131鉄禭e-131 + electron. The decay is first-order with a rate constant of 0.138 d鈭�1. All radioactive decay is first order. How many days will it take for 90% of the iodine鈭�131 in a 0.500 M solution of this substance to decay to Xe-131?
See all solutions

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