Ch.14 - Chemical EquilibriumWorksheetSee 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: PART A. What is dynamic equilibrium?(A) Dynamic equilibrium in a chemical reaction is the condition in which the rate of the forward reaction is higher than the rate of the reverse reaction.(B)Dynamic

Problem

PART A. What is dynamic equilibrium?

(A) Dynamic equilibrium in a chemical reaction is the condition in which the rate of the forward reaction is higher than the rate of the reverse reaction.

(B)Dynamic equilibrium in a chemical reaction is the condition in which the rate of the forward reaction equals the rate of the reverse reaction.

(C) Dynamic equilibrium in a chemical reaction is the condition in which the rate of the forward reaction is lower than the rate of the reverse reaction.


PART B. Why is it called dynamic?

(A) Dynamic equilibrium is called dynamic because the forward and reverse reactions are still occurring, however, they are occurring at the different rate.

(B) Dynamic equilibrium is called dynamic because the forward and reverse reactions are still occurring, however, they are occurring at the same rate.

Solution

At equilibrium, the rate of product formation is equal to the rate at which the reactants are being formed again. The concentration of the reactants and products are not necessarily equal. However, since the rate is equal, the concentration of the reactants and products remain constant.


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