Chemistry 11600
Fall 2014
Learning Objectives for
Equilibrium: The Extent of Chemical Reactions
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To describe the difference between “completion” for irreversible chemical reactions
and for reversible chemical reactions.
To describe a system at chemical equilibrium.
To describe the “position” of equilibrium.
To describe the law of chemical equilibrium (law of mass action).
To write an equilibrium constant expression for a reversible reaction in terms of
reactant and product concentrations or partial pressures (gases).
To calculate the value of the equilibrium constant for a reversible chemical reaction
given the equilibrium concentrations of all reactants and products.
To describe why the concentrations of the reactants and products do not change when
a chemical reaction has reached equilibrium.
To describe chemical equilibrium in terms of the rates of the forward and reverse
reactions.
To describe what information is provided by the value of the equilibrium constant
for a chemical reaction.
To calculate the value of Kp given the value of Kc (and vice versa).
To calculate the value of the reaction quotient, Q, given the concentrations or partial
pressures (gases) of reactants and products at any moment in time.
To describe how the value of the reaction quotient at any moment in time can be
used to:
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To describe two sets of conditions where a chemical reaction can reasonably be
treated as an irreversible reaction (i.e., single arrow).
To describe LeChatelier’s principle.
To describe the effect(s) on a system at chemical equilibrium when each of the
following is changed:
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determine whether or not a chemical reaction is at equilibrium.
determine in which direction the chemical reaction must proceed to reach
equilibrium.
concentration (either reactants or products)
pressure (amounts of either reactants or products; addition of an inert gas;
volume of the container)
temperature (reaction enthalpies)
To calculate the new equilibrium position attained when a change in concentration
of either a reactant or product is made to a system initially at equilibrium.
To describe and use the van’t Hoff equation.
Chemistry 11600
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Fall 2014
To describe the interplay between the rate of reaction and the magnitude of the
equilibrium constant for reversible chemical reactions.
To describe the “Haber-Bosch Process” and how the experimental conditions were
chosen to maximize the yield of ammonia.
To describe the effect of a catalyst on the equilibrium position for a reversible
chemical reaction.
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