15. Chemical Kinetics

Catalyst

Collision Theory

Energy Diagrams, Catalysts, and Reaction Mechanisms

One of the many remarkable enzymes in the human body 
is carbonic anhydrase, which catalyzes the interconversion 
of carbon dioxide and water with bicarbonate ion 
and protons. If it were not for this enzyme, the body could 
not rid itself rapidly enough of the CO2 accumulated by 
cell metabolism. The enzyme catalyzes the dehydration 
(release to air) of up to 107 CO2 molecules per second. 
Which components of this description correspond to the 
terms enzyme, substrate, and turnover number?

Potential Energy Diagrams - Chemistry - Catalyst, Endothermic & Exothermic Reactions

(c) Do catalysts
affect the overall enthalpy change for a reaction,
the activation energy, or both?

Catalysts | Kinetics | AP Chemistry | Khan Academy

Catalyst Concept 1

Why doesn’t a catalyst appear in the overall chemical equation 
for a reaction?

14.3 Reaction Mechanisms, Catalysts, and Reaction Coordinate Diagrams | General Chemistry

Catalyst Example 1

Many heterogeneous catalysts are deposited on high-surfacearea
supports. Why?

Which of the following statements is true regarding the energy diagram provided?&nbsp;i. The reaction is endothermic.ii. Activation energy would be less than + 10 kJ after a catalyst is added.iii. The reaction absorbs energy.iv. Activation energy would be greater than + 10 kJ after a catalyst is added.<img class="fr-dib"src="https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/images/7819a17f"style="width:300px;">a) I only &nbsp; &nbsp; &nbsp; &nbsp; &nbsp; &nbsp;b) II only&nbsp; &nbsp; &nbsp; c) I and III &nbsp; &nbsp; &nbsp; &nbsp; d) II, III and IV

In the following three instances, which choice is greener in a chemical process? Explain. (a) A reaction that can be run at 350 K for 12 h without a catalyst or one that can be run at 300 K for 1 h with a reusable catalyst.

Suppose that the reaction A¡products is exothermic and
has an activation barrier of 75 kJ>mol. Sketch an energy diagram
showing the energy of the reaction as a function of the
progress of the reaction. Draw a second energy curve showing
the effect of a catalyst.

Catalysis

Kinetics & the Catalyst

Comment on the following statement: “A catalyst increases 
the rate of a reaction, but it is not consumed because it 
does not participate in the reaction.”

Chemical Kinetics 3.6 - Catalysis

(a) Most commercial heterogeneous catalysts are extremely
finely divided solid materials. Why is particle size
important?

A catalyst will appear in the overall equation.

The change in rate experienced on the addition of a catalyst is due to a new alternate pathway for the reaction with a lower activation energy.

A catalyst changes the mechanism of a reaction.

Correct, the new mechanism has a lower activation energy.

A catalyst will increase the activation energy.

A catalyst is produced by the first step of a mechanism, then used in a later step.

A catalyst is completely consumed in the reaction.

 Review how a catalyst speeds up the rate of reaction. 

Which of the following is true about a catalyst?

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Intro to Chemical Kinetics

Chemical Kinetics is the study of factors affecting reaction rates, which examines the speed by which reactants are consumed to make products.

Average Rate of Reaction

Average (General) Rate is the change in the concentration of a compound over a period of time.

Arrhenius Equation

The Arrhenius Equation&nbsp;illustrates the temperature dependence of the rate constant k.&nbsp;

Rate Law

Rate Law represents an equation for a chemical reaction that connects the reaction rate with the concentrations or pressures of the reactants and the rate constant.&nbsp;

Factors Influencing Rates

There are 4 major factors that directly influence how fast or slow a reaction proceeds.

Stoichiometric Rate Calculations

When the rate of one compound is know, the rate of another compound is calculated through rate-to-rate comparison.

According to Collision Theory:chemical reaction is successful when 2 energetic reactants successfully collide.

Integrated Rate Law

When we include the variable of time to our Rate Law then we obtain the Integrated Rate Laws.&nbsp;

Catalyst is a substance that increases the rate of reaction by lowering the Activation Energy (Ea) of a reaction.

Instantaneous Rate

<div title="Page 1">&nbsp;Instantaneous Rate is the rate a reaction at any particular point in time.</div>

Reaction Mechanism

<div title="Page 1">A Reaction Mechanism is a step-by-step sequence of elementary steps by which an overall chemical change occurs.</div>

Half-Life

Half-Life is the time it takes for half&nbsp;of a reactant to decay in a certain time period.

Energy Diagrams

Energy Diagram represents a curved plot illustrating the energies of reactants, products and transition states of a reaction.

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