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: The rate law for the reaction: Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g) is rate = k [Cl2]1/2[CHCl3]3/4. The units for the rate constant are a) M−1/4 sec−1 b) M1/4 sec−1 c) M−5/4 sec−1 d) M−1/2 sec−1

Problem

The rate law for the reaction:

Cl2(g) + CHCl3(g) → HCl(g) + CCl4(g)

is rate = k [Cl2]1/2[CHCl3]3/4. The units for the rate constant are

a) M−1/4 sec−1

b) M1/4 sec−1

c) M−5/4 sec−1

d) M−1/2 sec−1

e) M−1 sec-1