Stoichiometry review 1. How many moles of hydrochloric acid will be required to produce 0.7 moles of hydrogen gas by the reaction with zinc? 2. How many moles of chlorine will be needed to produce 4.5 g of hydrogen chloride by reaction with hydrogen? 3. In an experiment, 32.1 g of potassium is reacted with oxygen to produce potassium oxide, K2O. a. Calculate the mass of the product produced. b. If the reaction took place at STP condition, calculate the volume of oxygen that reacted with potassium. 4. When 30.8 g of silver nitrate are reacted with enough sodium chloride. A double replacement reaction took place. Calculate the mass of silver chloride produced. 5. Given: 4 NH3 (g) + 5 O2 (g) ----> 6 H2O (g) + 4 NO (g) + 905 kJ ( at STP) a. What mass of water is produced when 4.6 g of NH3 is burned? b. What is the volume of NO produced when 4.6 L of oxygen reacts? c. How much energy is produced when 46.0 g of ammonia (NH3) reacts? 6. Aluminum metal reacts with copper (II) chloride to produce copper metal and aluminum chloride solution. If 0.50 g of aluminum is placed into a beaker containing 150 mL of 0.50 M copper (II) chloride solution, a. calculate the theoretical yield of this experiment? b. If the experiment produced 0.57 g of copper, what is the percent yield? 7. What volume of a 0.30 M solution of sodium carbonate is needed to neutralize 30.0 mL of a 0.45 M solution of sulfuric acid? 8. Calculate the mass of Iron (III) oxide (this is rust) produced by the reaction of 5.00x102 g of iron with oxygen from the air. 9. What mass of precipitate should form if 2.00 g of silver nitrate in solution is reacted with excess sodium sulfide solution. Hint: the silver sulfide is the precipitate. 10. Determine the mass of water vapour formed when 1.00 g of propane, C3H8 (g), is burned 11. Silver metal can be recovered from waste silver nitrate solutions by reactions with copper metal. What mass of silver can be obtained using 23 g of copper? 12. What volume of 0.250 M HCI is required to completely netralize 25.0 ml of 0.318 M NaOH? Hint: What is the balanced equation between HCI and NaOH? 13. student wants to put 50.0 L of hydrogen gas at STP into a plastic bag by reacting excess aluminum metal with 2.50 M sodium hydroxide solution according to the reaction: 2Al (s) + 2 NaOH (aq) + 2 H2O (l) --- > 2 NaAIO2 (aq) + 3 H2 (g) What volume of NaOH solution is required? 14. If 46.8 g of FeCl2, 14.0g of KNO3 and 40.0g of HCI are mixed and allowed to react according to the equation: 3FeCl2 + KNO3 + 4HCI ----- > 3FeCl3 +NO+ 2H2O + KCI a. Which chemical is the reactant in excess? b. What is the mass of KCl produced? c. How many grams of each "excess reactant" are actually present in excess? 15. The reaction SiO2 (s) + 4HF (g) ---- > SiF4 (g) + 2H2O (g) produces 2.50 g of H2O when 14.0 g of SiO2 is treated with small excess HF. a. What mass of SiF4 is formed? b. What is the percentage yield of the SiF4?
