1. Station #1 Rocket Fuel: The compound diborane (B 2 H 6 ) was at one time considered for use as a rocket fuel. How many grams of liquid oxygen would a rocket have to carry to burn 10 kg of diborane completely? The balanced chemical equation for this reaction is B 2 H 6 + 3 O 2  B 2 O 3 + 3 H 2 O

2. Station #2 Water in Space: In the space shuttle, the CO 2 that the crew exhales is removed from the air by a reaction within canisters of lithium hydroxide. On average, each astronaut exhales about 448 L of CO 2 daily. What mass of water will be produced when this amount of CO 2 reacts with an excess of LiOH? The balanced chemical equation for this reaction is : CO 2 (g) + 2 LiOH (s)  Li 2 CO 3 (aq)+ H 2 O (l)

3. Station #3 Determine the amount of LiOH required for a 7 day mission in space for three astronauts and one happy chimpanzee. Assume each passenger expels 20 mole of CO 2 per day. Note: the lithium hydroxide scrubbers are only 85% efficient. The balanced chemical equation for this reaction is CO 2 (g) + 2 LiOH (s)  Li 2 CO 3 (aq)+ H 2 O (l).

4. Station #4 Airbag design: The exact quantity of nitrogen gas must be produced in an instant. Assume that 65.1 L of N 2 gas are needed to inflate an airbag to the proper size. How many grams of NaN 3 must be included in the gas generator to generate this amount of N 2 ? The balanced chemical equation is 2 NaN 3 (s)  2 Na (s) + 3 N 2 (g)

5. Station #5 Fertilizer: Ammonia is commonly used for making fertilizer and is produced commercially by reacting nitrogen gas with hydrogen gas. If 15 g of hydrogen gas react, how many molecules of NH 3 will be produced?

6. Station #6 Fertilizer: Ammonium hydrogen phosphate, (NH 4 ) 2 HPO 4, a common fertilizer, is made from reacting phosphoric acid, H 3 PO 4, with ammonia. How much fertilizer will be produced from 84.3 grams of ammonia? (you must write the balanced chemical equation first)

7. Station #7 The following reaction shows the synthesis of zinc citrate, an ingredient in toothpaste, from zinc carbonate and citric acid: 3ZnCO 3 (s) + 2 C 6 H 8 O 7 (aq)  Zn 3 (C 6 H 5 O 7 ) 2 (aq) + 3 H 2 O (l) + 3CO 2 (g). How many grams of ZnCO 3 are required to produce 193.5 grams of Zn 3 (C 6 H 5 O 7 ) 2 ?

8. Station #8 Joseph Priestly is credited with the discovery of oxygen. He produced O 2 by heating mercury (II) oxide, HgO, to decompose it into its elements. What volume of oxygen could Priestly have produced if he had decomposed 517.84 g of mercury (II) oxide?

9. Station #9 A car battery produces electrical energy with the following chemical reaction: Pb (s) + PbO 2 (s) + 2H 2 SO 4 (aq)  2PbSO 4 (s)+2H 2 O (l). If the battery loses 0.34 kg of lead in this reaction, how many moles of lead (II) sulfate are produced?

10. Station #10 Water is sometimes removed from the products of a reaction by placing them in a closed container with excess P 4 O 10. Water is absorbed by the following reaction: P 4 O 10 + 6H 2 O  4H 3 PO 4. What mass of water can be absorbed by 1.00 × 10 2 g of P 4 O 10 ?

11. Station #11 Ethanol, C 2 H 5 OH, is made by fermenting and distilling starch crops, such as corn, and is considered a clean fuel because it burns in oxygen to produce carbon dioxide and water with few traces of pollutants. If 95.0 g of H 2 O are produced during the combustion of ethanol, how many grams of ethanol were present at the beginning of the reaction?

12. Station #12 Sulfur dioxide is one of the major contributors to acid rain. Sulfur dioxide can react with oxygen and water in the atmosphere to form sulfuric acid. If 50.0 g of sulfur dioxide from pollutants reacts with water and oxygen found in the air, what mass of sulfuric acid was formed in the process?