Question 1: When aluminum iodide is heated, it decomposes into its constituent elements. How many mg of starting material are required to produce 2.34 x 104 μg of the iodine if the reaction only results in an 84.2% yield? Give your answer in standard notation.

Question 2: How many grams of cobalt (III) carbonate would be needed to clean up (i.e. completely neutralize) a 4.53 L spill of 0.054 M phosphoric acid? Give the answer in standard notation.

Question 3: If a 5.67 g block of iron metal was left to rust (i.e. react with oxygen to form iron (III) oxide), and the final block had a mass of 6.98 g, what mass of rust was formed?

Question 4: What is the mass of precipitate that is formed when 482 nL of 3.54 M vanadium (V) nitrate is mixed with 8.37 x 10-6 mL of 1.32 M ammonium phosphate? Give your answer in standard notation.

Question 5: There are two solutes still in solution at the end of the reaction in the previous problem. What is the concentration of each solute at the end of that reaction? Give your answers in standard notation. Include the name of each solute with the concentration value.

Question 6: A student tried to recover all the gold metal from a 1.738 M solution of gold (III) sulfate by adding magnesium metal. They started with 450 gal of solution and added 65 lbs of magnesium metal. When the reaction was complete, they recovered 150 lbs gold metal. What was their percent yield?

Question 7: A 6754 mg block of copper metal is heated up to 198oC and then dropped into a cup containing 28.7 mL water. After a few minutes, both the metal and the water are at 56.2oC. What was the initial temperature of the water? The specific heat of copper is 0.383 J/goC.

Question 8: How much energy (in kJ) is required to convert a 4.0 lb block of ice at -24.5oF to steam at 121oC?

Question 9: What mass of propane (C3H8) must be burned (with just enough oxygen) to produce 23.4 mL of gas at 13.07 psi and 37oF? Give the answer in standard notation.

Question 10: A 458 mL closed container is filled with 458 mmHg oxygen gas and 0.557 cm3 of solid aluminum powder. The aluminum powder and oxygen are allowed to react until the limiting reagent is gone. What is the final pressure of in the container? Assume the temperature is constant at 76oF. The density of?aluminum is 2.70 g/mL. Give your answer in standard notation.

Question 11: A 2.65-quart tank of ammonia gas at 27.6 psi and 9.08oF is decomposed into hydrogen and nitrogen gases. If the final temperature is 67.0oC, what is the partial pressure (in mmHg) of the nitrogen gas in the tank at the end of the reaction? Give your answer in standard notation.

Question 12: A 1.78 gal canister contains 0.0045 lbs water at 14.6oC (the rest of the canister is an empty vacuum). How much energy is required to completely evaporate the water and raise the pressure to 16.2 psi?

Question 13: If 7.58 g of a group 2 metal is added to a sealed 500. mL container of hydrochloric acid at 35.0oC and 760 torr and the pressure increased to 16.77 atm after all the metal reacted, what is the metal? 

Question 14: If it took 939 kJ of energy to covert a block of ice at -12.0oC to steam at 102oC, how big (in g) was the block of ice?