Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

15. Chemical Kinetics

Arrhenius Equation

General Chemistry

15. Chemical Kinetics

Arrhenius Equation

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Multiple Choice

At 298 K, the decomposition of ammonia is catalyzed by tungsten. The activation energy for the catalyzed reaction is 163 kJ/mol. If in the absence of a catalyst, the activation energy is 335 kJ/mol, which of the following statements is true with reference to this reaction?

The catalyzed reaction has a lower activation energy, resulting in a faster reaction rate.

The catalyzed reaction has a higher activation energy, resulting in a slower reaction rate.

The catalyst increases the activation energy, making the reaction slower.

The catalyzed reaction and the uncatalyzed reaction have the same activation energy.

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Verified step by step guidance

Understand the concept of activation energy: Activation energy is the minimum energy required for a chemical reaction to occur. It is a barrier that reactants must overcome to transform into products.

Recognize the role of a catalyst: A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It typically works by lowering the activation energy needed for the reaction.

Compare the activation energies: In this problem, the activation energy for the catalyzed reaction is given as 163 kJ/mol, while the activation energy for the uncatalyzed reaction is 335 kJ/mol.

Analyze the effect of the catalyst: Since the activation energy is lower for the catalyzed reaction (163 kJ/mol) compared to the uncatalyzed reaction (335 kJ/mol), the catalyst makes it easier for the reaction to occur, thus increasing the reaction rate.

Conclude based on the comparison: The statement 'The catalyzed reaction has a lower activation energy, resulting in a faster reaction rate' is true because the catalyst reduces the activation energy, facilitating a quicker reaction.