1. A 95.3 gram sample of NOCl is placed in an evacuated 12.0 liter container at 35°C. What is the pressure in atmospheres inside the container? 2. CaCO3 (s) + HC2H3O2 (aq)  Ca(C2H3O2)2 (aq) + CO2 (g) + H2O (l) Which of the following changes to an experiment using the preceding reaction will most likely increase the rate of gas production? a) Decreasing the volume of HC2H3O2 solution used in the experiment b) Decreasing the concentration of the HC2H3O2 solution used in the experiment c) Decreasing the temperature at which the experiment is performed d) Decreasing the particle size of the CaCO3 (s) by grinding it into a fine powder 3. What is the pH for the following solutions? a. 0.000256 M HCl b. 1.26 x 10-8 M NaOH 4. HCl (g) + NH3 (g) ←→ NH4Cl (s) Predict the sign of the entropy change, ΔS, for the forward reaction. Explain your reasoning. 5. HCl (g) + NH3 (g) ←→ NH4Cl (s) The reaction is allowed to reach equilibrium. Additional solid NH4Cl is added to the reaction vessel. How will equilibrium be affected? Explain. 6. Which arrow represents a hydrogen bond in water? 7. H2 (g) + I2 (g)  2HI (g) KC = 50 at 450C. Which of the following will caused the system to produce more HI? a) Add more of HI (g) b) Increase the pressure inside the reaction vessel c) Add more I2 (g) d) Increase the volume of the reaction vessel 8. Which of the following represents a Bronsted-Lowry acid-base pair? a) H2C2O4 (aq) and C2O42- (aq) b) HC2O41- (aq) and C2O42- (aq) c) HC2O41- (aq) and H2O (aq) d) H3O+ (aq) and OH1- (aq) 9. What volume of 0.25 M HNO3 is needed to fully neutralize 16 mL of 0.15 M Ca(OH)2? 10. Which of the following reactions is not spontaneous at low temperatures, but is spontaneous at high temperatures? Reaction H (kJ/mol) S (J/molK) a) 2CO (g) + O2 (g)  2 CO2 (g) -566 -173 b) 2H2O (g)  2H2 (g) + O2 (g) 484 90.0 c) 2N2O (g)  2N2 (g) + O2 (g) -164 149 2+ d) PbCl2 (s)  Pb (aq) + 2Cl (aq) 23.4 -12.5 11. PCl5 (g)  PCl3 (g) + Cl2 (g) As the forward reaction progresses toward equilibrium, the rate of the forward reaction ___. a) increases until it becomes the same as the reverse reaction rate at equilibrium b) stays constant before and after equilibrium is reached c) decreases to become a constant rate at equilibrium. d) Decreases to become zero at equilibrium Use the following table to answer the questions Concentrations pH of substance 1 pH of substance 2 pH of substance 3 0.010 3.44 2.00 11.08 0.050 3.09 1.30 11.42 0.10 2.94 1.00 11.58 12. Which of the substances is a base? a) substance 1 b) substance 2 c) substance 3 13. Which of the substances is a strong acid? a) substance 1 b) substance 2 c) substance 3 heat + SO2 (g) + Cl2 (g)  SO2Cl2 (g) The KC value for the reaction at 401K is 2.20. 14. Does this reaction favor the reactants or the products? Justify your answer. 15. If 2.50 g of SO2 and 1.75 g of Cl2 are reacted, a. What mass of SO2Cl2 is created? b. What is the limiting reactant? 16. Draw a diagram showing how LiCl is dissolved in water. Your drawing must include  the identity of the ions (symbol and charge)  the arrangement and proper orientation of the water molecules.  Use only one LiCl formula unit and a maximum of 10 water molecules 17. What mass of KBr (molar mass = 119 g/mol) is required to make 250. mL of a 0.400 M KBr solution? a) 1.19 g b) 2.50 g c) 11.9 g d) 47.6 g 18. Which of the following reactions will shift to the left when the pressure on the system is increased? a) 2Mg (s) + O2 (g)  2MgO (s) b) SF4 (g) + F2 (g)  SF6 (g) c) N2 (g) + 3 H2 (g)  2NH3 (g) d) SO2Cl2 (g)  SO2 (g) + Cl2 (g) 19. 2HI (g) H2 (g) + I2 (g) The Hrxn = -26 kJ/mol. Which of the following is the mass of HI (g) that must decompose to release 500. kJ of energy? a) 203 g b) 2440 g c) 2460 g d) 4920 g 20. Which of the following actions would increase the boiling point of a sample of water in an open container? a) Adding 15 grams of solid calcium chloride b) Removing some of the liquid in the container c) Moving the container to a higher altitude d) Adding some liquid to the container 21. How many milliliters of 12.0 M HCL must be diluted to obtain 2.00 L of a 3.00 M HCl? 22. Which solution has the lower freezing point and why? 0.10 M oxalic acid, H2C2O4 or 0.10 M magnesium nitrate, Mg(NO3)2 23. State the Collision Theory. 24. The energy diagram for the reaction Z + X  Y is shown above. The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences? 25. CaCO3 (s)  CaO (s) + CO2 (g) If 25.0 g of calcium oxide was made and the theoretical yield for the reaction is 35.6 g, what is the percent yield? 26. A balloon contains 2.5 L of gas at 27C. If the balloon is heated to 30C, the volume will ___ a. Increase. b. Decrease c. Stay the same 27. A balloon contains 2.5 L of gas at a pressure of 1.25 atm. If the balloon’s volume is changed to 1.5 L, the pressure inside the balloon will ___. a. Increase b. Decrease c. Stay the same 28. If 20.0 g of hydrogen peroxide decomposes, what volume of oxygen gas can be made at STP? 2H2O2 (l)  2H2O (g) + O2 (g)