Table of contents

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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

Rate Law

General Chemistry

15. Chemical Kinetics

Rate Law

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Multiple Choice

Based on the given two-step mechanism for the formation of 2NO2(g) from NO(g) and O2(g), what is the rate law for the overall reaction?

Rate = k[NO][O2]

Rate = k[NO2]^2

Rate = k[NO3][NO]

Rate = k[NO]^2[O2]

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Verified step by step guidance

Identify the overall reaction by combining the elementary steps of the given mechanism. The mechanism typically involves intermediate species that are not present in the overall balanced equation.

Determine the rate-determining step (RDS) in the mechanism. The RDS is the slowest step and dictates the rate law for the overall reaction.

Write the rate law based on the molecularity of the RDS. The molecularity refers to the number of reactant molecules involved in the RDS, which directly influences the rate law expression.

If the RDS involves an intermediate, express the intermediate in terms of the reactants using the equilibrium assumption or steady-state approximation, depending on the mechanism details.

Combine the expressions to form the rate law for the overall reaction, ensuring that it is expressed in terms of the initial reactants only, without intermediates.