Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Consider the reaction mechanism NO2(g) + Cl2(g) → ClNO2(g) + Cl(g)     SlowNO2(g) + Cl → ClNO2(g)                       FastWhat is the predicted rate law for this mechanism?a) Rate = k[NO2][Cl2][Cl]b


Consider the reaction mechanism 

NO2(g) + Cl2(g) → ClNO2(g) + Cl(g)     Slow

NO2(g) + Cl → ClNO2(g)                       Fast

What is the predicted rate law for this mechanism?

a) Rate = k[NO2][Cl2][Cl]

b) Rate = k[NO2][Cl]

c) Rate = k[NO2]2[Cl2]

d) Rate = k[NO2][Cl2]

e) Rate = k[NO2]2[Cl2][Cl]−1


When a reaction mechanism is given, the rate law can be determined using the slow step in the reaction mechanism.

 rate law only involves the reactants
▪ the coefficients of the reactants in the slow step are the order of the reaction with respect to that reactant
▪ Rate Law has a general form of:

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