1. Use the letter range on the graph to answer the following: Energy of Reactant Energy of Activated Complex Energy of Products Ea Show how to calculate the ΔH Is the reaction Endothermic or Exothermic? Which letter(s) value would change if a catalyst were added? 2. Indicate the values, in kJ, for the following: Energy of the Reactants Energy of Activated Complex Energy of the Products Ea ΔH Is this Endothermic or Exothermic Ea of the reverse reaction If an inhibitor was added that changed the Activation Energy by 20kJ, what would the new Activation Energy be? 3. How will the following changes affect the reaction rate for the reaction A + B → AB? Answer with Increases or Decreases. Removing B from the system. Crushing A into a powder. Warming the system. Adding more A to the system. Putting the system into an ice bath. Decreasing the pressure on the system. 4. Write the expression for the equilibrium constant Keq for the reactions below and calculate K based on the concentrations given. Then evaluate that Keq and state which direction the reaction favors, forward (products) or reverse (reactants). N2(g) + 3H2(g) ↔ 2NH3(g) Direction Favored [NH3]=0.01M 2KClO3(s) ↔ 2KCl(s) + 3O2(g) Direction Favored [O2]=0.05M H2O(l) ↔ H+(aq) + OH-(aq) [H+]=1x10-8M [N2]=0.02M [H2 ]=0.02M [OH-]=1x10-6M Direction Favored 2CO (g) + O2(g) ↔ 2CO2(g) [CO]=2M Direction Favored [O2]=1.5M [CO2]=3M 5. For the reaction below, indicate which direction the equilibrium would shift when the following changes take place. Answer with forward or reverse. CH4(g) + 2H2S(g) + 110kJ/mol ↔ CS2(g) + 4H2(g) Decrease the concentration of dihydrogen sulfide. Increase the pressure on the system. Increase the temperature of the system. Decrease the concentration of carbon disulfide. Decrease the concentration of methane
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