The following diagrams represent a hypothetical reaction A ⇋ B, with A represented by white spheres and B represented by black spheres. The sequence from left to right represents the system as time passes.a. Do the diagrams indicate that the system has reached equilibrium? (Circle one) ( Yes / No )b. Use concentration and reaction rate to describe what is occurring when a system has reached dynamic equilibrium.

Use the given equilibrium constant to identify it's corresponding chemical equation assuming every reactant and product are in the gas phase.   Keq = ([NH3]4[O2]3)/([N2]2[H2O]6)

Which is the appropriate description to show the effect of a catalyst on the reaction rate and equilibrium in a reversible reaction: Reactants › Products O• The rate of the forward reaction is increased. • The rate of the reverse reaction is decreased 0 •The equilibrium position is displaced to the right O • The rate of the forward reaction is increased. The rate of the reverse reaction is increased The equilibrium position is unchanged. • The rate of the forward reaction is increased. 0 •The rate of the reverse reaction is unchanged • The equilibrium position is displaced to the right • The rate of the forward reaction is unchanged. The rate of the reverse reaction is unchanged The equilibrium position is unchanged. Suppose that an exothermic reaction, Reactants < › Products, is at equilibrium. According to Le Chatelier's Principle, if the reaction temperature is increased, in which direction will the equilibrium be displaced? O The equilibrium will be displaced toward the…

7. Given the following equilibrium systems, note the direction the equilibrium will shift [→,-, NC, no change] when the named "stress" is applied. 2 NH3(g) + 92.5 kJ a 1 2 3 4 5 6 7 Stress Remove N2 (g) Add NH3 (9) Remove H2 (9) Remove NH3 (g) Add O2 (g) Decrease Pressure Add Heat N2(g) + 3 H2 (g) Equilibrium Shift

Consider the reaction. NaC2O2H3(s) <--- H2O ------> NaC2O2H3(aq), which is at equilibrium in an open flask in the lab at room temperature. You add more water to the equilibrium mixture. When the system reestablishes equilibrium, what has changed?  a. the concentration of NaC2H3O2(aq) does not change b. heat is produced c. the concentration of NaC2H3O2(aq) decreases d. the concentration of the water increases

1. The reaction shown below is carried out at various temperatures and the value of Kc determined. Draw particulate representations that show the relative amounts of each reactant and product that would roughly correspond to the value of K. Legend = PC13 = Cl₂ ∞ = = PC15 PC13 (g) + Cl2 (g) = PC15 (g) Magnitude of K Particulate diagram of equilibrium mixture 1 x 10 -3 1 x 105

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.

Label the following statements as true or false.    1) If Kc=5 for the reaction A + B <--> AB, then AB <--> A + B has a Kc=0.2   2)  When a system is at equilibrium, the reactants and the products of the reaction will be equal in concentration.    When Q > Kc, the reaction shifts to the left to reduce stress on the system.    3) When a system is at equilibrium, the reaction rate of the forward reaction is less than to the reaction rate of the reverse reaction.    4) When Q < Kc, the reaction shifts to the left to reduce stress on the system.    5) For a reversible reaction, the ΔH of the forward reaction is equal in magnitude but opposite in sign to the ΔH of the reverse reaction.

QUESTION 4 Adding a catalyst to an equilibrium system will:     produce more products at equilibrium.     produce more reactants at equilibrium.     not change the amount of reactants or products at equilibrium.

When a system is a dynamic equilibrium, A no reactions are occurring B a reaction is occurring in only one direction C the rates of the forward and reverse reactions are equal D all of the reactants have been converted to products