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 Arrhenius equation describes the relationship between the rate constant,  k, and the energy of activation, Ea. k = Ae–Ea / RT In this equation, A is an empirical constant, R, is the ideal-gas co

Problem

The Arrhenius equation describes the relationship between the rate constant,  k, and the energy of activation, Ea.

k = Ae–Ea / RT

In this equation, A is an empirical constant, R, is the ideal-gas constant, e is the base of natural logarithms, and T is the absolute temperature. According to the Arrhenius equation,

(A) at constant temperature, reactions with lower activation energies proceed more rapidly.

(B) at constant temperature, reactions with lower activation energies proceed less rapidly.

(C) at constant energy of activation, reactions at lower temperatures proceed more rapidly.

(D) at constant energy of activation, reactions with smaller values of A proceed more rapidly.