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: Predict and calculate the effect of concentration changes on an equilibrium system. Some SbCl5 is allowed to dissociate into SbCl3, and Cl2 at 521 K. At equilibrium, [SbCl5] = 0.163 M, and [SbCl3] = [

Problem

Predict and calculate the effect of concentration changes on an equilibrium system. 

Some SbCl5 is allowed to dissociate into SbCl3, and Cl2 at 521 K. At equilibrium, [SbCl5] = 0.163 M, and [SbCl3] = [Cl2] = 6.39 x 10-2 M. Additional SbCl5 is added so that [SbCl5]new = 0.287 M and the system is allowed to once again reach equilibrium. 

SbCl(g) ⇌ SbCl3 (g) + Cl2 (g) K = 2.50 x 10-2 at 521 K 

(a) In which direction will the reaction proceed to reach equilibrium? 

(b) What are the new concentrations of reactants and products after the system reaches equilibrium?