1. Determine the oxidation state of each element in the following compounds:
  2. Cr2O72-
  3. NO2
  4. SO42-
  5. MnO2
  6. H2P2O7-2
  7. BrF5
  8. Define reduction and oxidation.
  9. Identify the species being oxidized and reduced in each of the following reactions:
  1. 2 Cr+ + Sn4+----> Cr3+ + Sn2+
  2. 3 Hg2+ + 2 Fe ----> 3 Hg2 + Fe 3+
  3. 2 As + 3 Cl2----> 2 AsCl3
  1. Using the EMF series, decide which of the following redox reactions is spontaneous.
  2. 3 Ag + Au3+ ----> Au + 3 Ag+
  3. Au + 3 Ag+----> Ag+ Au3+
  4. Write half reactions for each redox reaction
    (# electrons lost must equal # of electrons gained)
    2Li+NiSO4Li2SO4+Ni
    4Al+ 3Mn(NO3)44Al(NO3)3+3Mn
  5. Balance following net ionic equation:
    Al0+Mn7Al3+Mn2
  1. If you were to decrease volume to ¼ of initial volume. What would happened to the pressure assuming that everything else would stay constant?
  2. If I have 4.0 moles of a gas at a pressure of 5.6 atm and a volume of 12 liters, what is the temperature?
  3. A sample of nitrogen gas, N2, is collected in a100 mL container at a pressure of 688 mm Hg and a temperature of 565 °C. How many grams of nitrogen gas are present in this sample?( 1 atm=760mm)
  4. Consider a container with 1.00 mole of gas at 120K and initial pressure P. The temperature is double to 240K and ____ number of moles of gas (at 240K) are added to the container until the pressure reaches 4P.
  5. At what temperature Celsius will 19.4 g of molecular oxygen, O2, exert a pressure of n n1820 mm Hg in a 5.12 L cylinder?(1atm =760mm)
  6. Define:
  7. Solution:
  8. Solvent:
  9. Solute:
  10. Describe how you would prepare 250.0 mL of a 0.300 M solution of KCl from solid KCl and water. (AKA how many grams of KCl you need?)
  11. A solution is prepared by mixing 100.0 g of glucose (C6H12O6) with enough water to make 500.0 mL of solution. Calculate the molarity of the solution.
  12. Calculate the percent by mass of a solution that is prepared by mixing 35.0 grams of ethanol (C2H5OH) and 150.0 grams of water.
  13. It takes 83 mL of a 0.45 M NaOH solution to neutralize 235 mL of an HCl solution. What is the concentration of the HCl solution?