Butane, C4H10 can be burned in oxygen gas according

1. Butane, C4H10 can be burned in oxygen gas according to the reaction below. 2C4H10 (g) + 13O2 (g)  8CO2 (g) + 10H2O (v)a) How many moles of carbon dioxide are produced when6. 8 moles of butane are completely burned? . . . . . . . . . . . . . . . . . . . . _________________b) Assuming complete combustion, what mass of waterwould be produced from 75. 0 mol of oxygen? . . . . . . . . . . . . . . . . . . . . _________________c) How many moles of oxygen would be required to produce1. 561 kg of pure carbon dioxide gas at STP?. . . . . . . . . . . . . . . . . . . . . . . . _________________d) If 6. 8 moles of propane (C3H8) were burned what minimum mass of oxygen gas would be required for complete combustion. You must write a balanced chemical equation similar to that found on the top of this page to solve this question. (5)BONUS: What mass of water could be formed from 75 g of oxygen and 75 kg of propane. 2. In the reaction for question 1 above, a tank contained a mixture of butane and non reactive krypton. The two gases together had a mass of 805 g. When completely burned, 1. 35 kg of carbon dioxide was produced. Determine the percent by mass krypton in the mixture. (10)3. Consider the following reaction: 2 Al + 3 I2 ——> 2 Al(I)3a) Determine the limiting reagent and the theoretical yield of the product in grams if one starts with 1. 20 mol Al and 2. 40 mol iodine. (4)b) Determine the theoretical yield of the product in grams if one starts with 1. 20 g Al and 2. 40 g iodine. How many grams of Al are left over in part b? (6)8. In the thermite reaction aluminum reacts with rust quite dramatically. The reaction is : 2 Al + Fe2O3 = 2 Fe + Al2O3. a) If 10 g each of Al and Fe2O3 are used how much Fe should be produced when the limiting reactant is exhausted? (8)b) What is the percent by mass yield of iron if only 3. 0 g of iron is recovered from the original 10 g of iron (iii) oxide? (2)9. TNAZ is a dense (1. 832 g/cm3) explosive with the proper name 1,3,3-trinitroazetidine, C3H4N4O6, often just abbreviated as “TNAZ”. When TNAZ detonates, it produces only carbon dioxide, carbon monoxide, water and nitrogen, all in the gaseous state. Like most pure substances that are explosive, the TNAZ molecule contains all of the oxygen it needs for the detonation reaction, so no reactants other than the solid explosive are involved (it can explode in outer space!). a) Given this information, write a balanced chemical reactionfor the detonation of TNAZ. Hint: just use some (small number) coefficients on the product side of the reaction. b) What is the molar mass of TNAZ?c) The “oxygen balance” is an important property of explosives. What is the percent by mass of oxygen in a sample of TNAZ?d) How many moles of TNAZ are there in a sample of the material that has a volume of 1. 00 cm3?e) If a 1. 00 cm3 sample of TNAZ is detonated, how many grams of CO2 are produced? (4)f) What mass of TNAZ would have to be detonated to produce 175 g of water vapor? What if only 137 g of H2O was produced—what would be the percent yield of the reaction? (6)

Butane, C4H10 can be burned in oxygen gas according

1. Butane, C4H10 can be burned in oxygen gas according to the reaction below. 2C4H10 (g) + 13O2 (g)  8CO2 (g) + 10H2O (v)a) How many moles of carbon dioxide are produced when6. 8 moles of butane are completely burned? . . . . . . . . . . . . . . . . . . . . _________________b) Assuming complete combustion, what mass of water would be produced from 75. 0 mol of oxygen? . . . . . . . . . . . . . . . . . . . . _________________c) How many moles of oxygen would be required to produce 1. 561 kg of pure carbon dioxide gas at STP?. . . . . . . . . . . . . . . . . . . . . . . . _________________d) If 6. 8 moles of propane (C3H8) were burned what minimum mass of oxygen gas would be required for complete combustion. You must write a balanced chemical equation similar to that found on the top of this page to solve this question. (5)BONUS: What mass of water could be formed from 75 g of oxygen and 75 kg of propane. 2. In the reaction for question 1 above, a tank contained a mixture of butane and non reactive krypton. The two gases together had a mass of 805 g. When completely burned, 1. 35 kg of carbon dioxide was produced. Determine the percent by mass krypton in the mixture. (10)3. Consider the following reaction: 2 Al + 3 I2 ——> 2 Al(I)3 a) Determine the limiting reagent and the theoretical yield of the product in grams if one starts with 1. 20 mol Al and 2. 40 mol iodine. (4)b) Determine the theoretical yield of the product in grams if one starts with 1. 20 g Al and 2. 40 g iodine. How many grams of Al are left over in part b? (6)8. In the thermite reaction aluminum reacts with rust quite dramatically. The reaction is : 2 Al + Fe2O3 = 2 Fe + Al2O3. a) If 10 g each of Al and Fe2O3 are used how much Fe should be produced when the limiting reactant is exhausted? (8)b) What is the percent by mass yield of iron if only 3. 0 g of iron is recovered from the original 10 g of iron (iii) oxide? (2)9. TNAZ is a dense (1. 832 g/cm3) explosive with the proper name 1,3,3-trinitroazetidine, C3H4N4O6, often just abbreviated as “TNAZ”. When TNAZ detonates, it produces only carbon dioxide, carbon monoxide, water and nitrogen, all in the gaseous state. Like most pure substances that are explosive, the TNAZ molecule contains all of the oxygen it needs for the detonation reaction, so no reactants other than the solid explosive are involved (it can explode in outer space!). a) Given this information, write a balanced chemical reactionfor the detonation of TNAZ. Hint: just use some (small number) coefficients on the product side of the reaction. b) What is the molar mass of TNAZ?c) The “oxygen balance” is an important property of explosives. What is the percent by mass of oxygen in a sample of TNAZ?d) How many moles of TNAZ are there in a sample of the material that has a volume of 1. 00 cm3?e) If a 1. 00 cm3 sample of TNAZ is detonated, how many grams of CO2 are produced? (4)f) What mass of TNAZ would have to be detonated to produce 175 g of water vapor? What if only 137 g of H2O was produced—what would be the percent yield of the reaction? (6)