Question

Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s) + H2O(g) Kc = for the following reaction: CO(g) + H2(g) 250; (g) [1.5pts] 5. Determine the value of Keq for the reaction 2502(g) + O2(g) where [SO] -0.065M, [O2] = 0.554 M, [SO] -0.045 M 6. State in which direction (+, +, or no effect) the above reaction will proceed in response to the following changes: [2.5 pts] 1 N2(g) + 3H2(g) = 2NH3(g) + Heat a. Increase in gas pressure b. Decrease in concentration of Hz c. Increase in Temperature d. Addition of a catalyst e. Decrease in concentration of NH3 7. Write the balanced chemical reaction that for the following expression for Ke and where Ag (s) is a reactant and AgCl (s) is a product: [1.5pts] [CI, (g)]

Answer 1

Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: frue False [1pt] 2. For the reaction C(s) + H2O(g) - CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left no effect True False [1pt] 3. Define the following terms: [1.5pts] 2. Activation Energythe minimum amount of energy required by the substance to attain the threshold enery barrier b. Exothermic Reaction A chemical reaction, in which heat is evolved during the reaction is called exothermic reaction c. Equilibrium chemically equilibrium in a reversible reaction is the state at which both forward and backward reactions and two opposing reactions occur at the same speed 4. Determine the equilibrium constant Key for the following reaction: [1 pt) C(s) + H2O(g) CO(g) + H2(g) Keq = [H2] [Co]/[H20] 250; (g) [1.5pts] 5. Determine the value of Keq for the reaction 2502(g) + O2(g) where [SO2] = 0.065M, [02] = 0.554 M, [SO3] = 0.045 M Keq = [S03]2/[02] [S02)2 = (0.045)2 / (0.554) (0.065)2 = 0.865 6. State in which direction (+, +, or no effect) the above reaction will proceed in response to the following changes: [2.5 pts] 1 N2(g) + 3H2(g) = 2NH3(g) + Heat a. Increase in gas pressure b. Decrease in concentration of H2 c. Increase in Temperature d. Addition of a catalyst e. Decrease in concentration of NH3 NO EFFECT 7. Write the balanced chemical reaction that for the following expression for Ke and where Ag (s) is a reactant and AgCl (s) is a product: [1.5pts] 2Ag(s) + Cl2(g) <---------> 2AgCl(s) op [CI, (g)]