For a particular reaction, which of the following statements is TRUE? O Keg for the reverse reaction is equal to negative Kea (-Ke) for the forward reaction. All of the statements are true. O Dynamic equilibrium indicates that reactant and product concentrations are equal. O A reaction quotient that is smaller than Keg means that the reaction will favor reactants. O When the reverse rate for a reaction equals its forward rate, dynamic equilibrium has been reached.

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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…

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

In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. For an exothermic reaction there is an increase in temperature.

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.

Consider the exothermic reaction: C2H4(g) + I2(g) = C2H412(g) In trying to maximize the amount of C2H412 produced, which of the following will not work? Assume that the reaction mixture reaches equilibrium. O increasing the temperature O decreasing the volume of the reaction vessel O increasing the amount of C2H4 O adding more l2

The following reaction is exothermic: 3A(g) B(g) + C(g) Gaseous argon is added to the equilibrium mixture without change in volume or temperature. Predict the effect of the possible stress mentioned directly above on the reaction mixture by selecting the correct phrase bel shift right to attain chemical equilibrium no shift to attain chemical equilibrium shift left to attain chemical equilibrium Onot enough information to answer question Previous DELL II O O O O

Which of the following is true for a system whose equilibrium constant is much greater than one? The reaction mixture contains mostly products at equilibrium. The reaction mixture contains mostly reactants at equilibrium. O The rate of reaction is very fast. The moles of reactants and products are relatively similar at equilibrium. Both A and C.

explain how it can be concluded from the shape of the Job's graph whether a reaction is an equilibrium or it is a complete 1 way reaction.