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: Using the Equilibrium constant The reversible chemical reaction A + B ⇌ C + D has the following equilibrium constant. Kc = [C][D]/[A][B] = 2.7 Part A Initially, only A and B are present, each at 2.00

Problem

Using the Equilibrium constant 

The reversible chemical reaction 

A + B ⇌ C + D 

has the following equilibrium constant. 

Kc = [C][D]/[A][B] = 2.7 

Part A 

Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?

Express the molar concentration numerically using two significant figures.