Chapter 14
Chemical Equilibrium
, Learning Objecti
• Distinguish, describe, and explain the nature of a dynamic equilibrium
• Explain the basics of equilibrium law
• Write and convert between equilibrium laws based on molar concentration and gas
pressures
• Understand and explain why solids and pure liquids are not included in equilibrium l
• Interpret the value of the equilibrium constant as an indicator of the position of equ
• Use the Le Châtelier's principle and the reaction quotient, Q, to interpret where a sy
in relation to equilibrium
• Describe experiments to determine the equilibrium constant and how to use the da
these experiments
• Use tabulated values of equilibrium constants and experimental data to calculate th
equilibrium concentrations (or pressures of all species in an equilibrium mixture)
,• Distinguish, describe, and explain the nature of a dynamic
equilibrium
• Explain the basics of equilibrium law
• Understand and explain why solids and pure liquids are no
included in equilibrium laws
• Interpret the value of the equilibrium constant as an
indicator of the position of equilibrium
, Dynamic Equilibrium in Chemical
Systems
• Chemical equilibrium exists when
• Rates of forward and reverse reactions are equal
• Reaction appears to stop
• Concentration of reactants and products do not
change over time
• Remain constant
• Both forward and reverse reaction never
cease
• Equilibrium signified by double arrows ( )
Chemical Equilibrium
, Learning Objecti
• Distinguish, describe, and explain the nature of a dynamic equilibrium
• Explain the basics of equilibrium law
• Write and convert between equilibrium laws based on molar concentration and gas
pressures
• Understand and explain why solids and pure liquids are not included in equilibrium l
• Interpret the value of the equilibrium constant as an indicator of the position of equ
• Use the Le Châtelier's principle and the reaction quotient, Q, to interpret where a sy
in relation to equilibrium
• Describe experiments to determine the equilibrium constant and how to use the da
these experiments
• Use tabulated values of equilibrium constants and experimental data to calculate th
equilibrium concentrations (or pressures of all species in an equilibrium mixture)
,• Distinguish, describe, and explain the nature of a dynamic
equilibrium
• Explain the basics of equilibrium law
• Understand and explain why solids and pure liquids are no
included in equilibrium laws
• Interpret the value of the equilibrium constant as an
indicator of the position of equilibrium
, Dynamic Equilibrium in Chemical
Systems
• Chemical equilibrium exists when
• Rates of forward and reverse reactions are equal
• Reaction appears to stop
• Concentration of reactants and products do not
change over time
• Remain constant
• Both forward and reverse reaction never
cease
• Equilibrium signified by double arrows ( )
