How are the amounts of products, according to Le Châtelier's principle, changed when a large excess of a gaseous reactant is added to a reaction system at equilibrium? O The amounts of products will increase. O The amounts of products will be constant. O The amounts of products will decrease. O The amounts of products will fluctuate.

Define equilibrium in terms of  a)reaction rates   -Forward reaction rate = reverse reaction rate b)changes in observable properties   -There are no observable changes c)energy and energy changes   -Energy has become stable (no longer giving off or taking in heat)

Decide whether each of the following statements is true or false.  If false, change the wording of the statement to make it true.   a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction.  d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.

In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change.  The concentration of one or more of the products is increased.