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Chapter 12: Q80E. (page 713)

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

Short Answer

Expert verified

(a) Reaction diagram (b) is a catalyzed reaction.

(b) Reaction diagram (b) is a catalyzed reaction.

Step by step solution

01

Definition of Catalyst

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

  • A catalyst increases the rate of reaction.
  • Catalyst accelerates the rate of a reaction by decreasing the activation energy.
  • Catalyst is regenerated during the reaction.
02

(a) Reaction diagram (b) uses a catalyst

  • The two reaction diagrams depict the same reaction, one with a catalyst and another without a catalyst.
  • We can ignore the energy aspect of the diagram as the catalyst does not involve in affecting the energy of the reactant or product.
  • But we can notice a small change in the transition state, which is lower in diagram (b) than in diagram (a).

This indicates the presence of a catalyst in diagram (b).

03

(b) Reaction diagram (b) uses a catalyst 

  • The two reaction diagrams depict the same reaction, one with a catalyst and another without a catalyst.
  • We can notice a small change in the transition state, which is lower in diagram (b) than in diagram (a).

This indicates the presence of a catalyst in diagram (b).Thus, the reaction diagram (b) is catalyzed among both pairs of reaction diagrams (a) and (b).

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Most popular questions from this chapter

The rate constant for the decomposition of acetaldehyde, \({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{CHO}}\), to methane, \({\bf{C}}{{\bf{H}}_{\bf{4}}}\), and carbon monoxide, CO, in the gas phase is 1.1 × 10−2 L/mol/s at 703 K and 4.95 L/mol/s at 865 K. Determine the activation energy for this decomposition.

Usethe data provided to graphically determine the order and rate constant of the following reaction: \({\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{C}}{{\bf{l}}_{\bf{2}}} \to {\bf{S}}{{\bf{O}}_{\bf{2}}}{\bf{ + C}}{{\bf{l}}_{\bf{2}}}\)

Time(hr)

0

5.00*\({\bf{1}}{{\bf{0}}^{\bf{3}}}\)

1.00*\({\bf{1}}{{\bf{0}}^{\bf{4}}}\)

1.50*\({\bf{1}}{{\bf{0}}^{\bf{4}}}\)

2.50*\({\bf{1}}{{\bf{0}}^{\bf{4}}}\)

3.00*104

4.00*104

\({\bf{(S}}{{\bf{O}}_{\bf{2}}}{\bf{C}}{{\bf{l}}_{\bf{2}}}{\bf{)}}\)(M)

0.100

0.0896

0.0802

0.0719

0.0577

0.0517

0.0415

Determine which of the two diagrams here (both for the same reaction) involves a catalyst, and identify the activation energy for the catalyzed reaction:

The rate law for the reaction: \({{\bf{H}}_{\bf{2}}}\) (g) + 2\({\bf{NO}}\) (g) ⟶\({\bf{N}}2{\bf{O}}\) (g) + \({{\bf{H}}_{\bf{2}}}\)O(g) has been determined to be rate = k(\({\bf{NO}}\))2 (\({{\bf{H}}_{\bf{2}}}\)). What are the orders with respect to each reactant, and what is the overall order of the reaction?

Compare the functions of homogeneous and heterogeneous catalysts.
See all solutions

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