Which of the changes listed has no effect on the equilibrium for the following reversible reaction? SO3(g) + NO(g) + heat = SO2(g) + NO2(g) decrease volume. Add helium gas. Increase volume. Add a catalyst. All of the above

Indicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Removal of a reactant from the equilibrium mixture b. Decrease in the systems total pressure c. Decrease in the systems temperature d. Addition of a catalyst to the equilibrium mixture

Indicate whether or not each of the following changes would affect the value of a systems equilibrium constant. a. Addition of a product to the equilibrium mixture b. Increase in the systems total pressure c. Increase in the systems temperature d. Addition of both a reactant and a product to the equilibrium mixture

The gaseous reaction 2HBr(g)H2(g)+Br2(g) is endothermic. Tell which direction the equilibrium will shift for each of the following: a.Some H2 is added. b.The temperature is increased. c.Some Br2 is removed. d.A catalyst is added. e.Some HBr is removed. f.The temperature is decreased, and some HBr is removed.

Tell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. LiOH(s)+CO2(g)LiHCO3(s)+heat; CO2 is removed. b. 2NaHCO3(s)+heatNa2O(s)+2CO2(g)+H2O(g); The system is cooled. c. CaCO3(s)+heatCaO(s)+CO2(g); The system is cooled.

Consider the following equilibrium system. N2(g)+O2(g)2NO(g) a. Write the chemical equation for the forward reaction. b. Write the chemical equation for the reverse reaction.

For the reaction C6H6(g)+3H2(g)C6H12(g)+heat determine in what direction the equilibrium will be shifted by each of the following changes. Decreasing the concentration of H2 a. Increasing the concentration of C6H6 b. Decreasing the temperature c. Increasing the pressure by decreasing the volume of the container

Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-83, which of the diagrams represents the equilibrium mixture if the numerical value of the equilibrium constant is 9.0?

. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?

Use Le Chteliers principle to predict the direction of equilibrium shift in the following equilibria when the indicated stress is applied: a. 2A+B+heatC; some A is removed. b. 2A+B+heatC+D; the system is cooled. c. N2O42NO2; some NO2 is removed.