Reference no: EM132439086

Question 1: When ethane (C2H6) burns, it produces carbon dioxide and water: 2C2H6 (g) + 7O2 (g) --> 4CO2 (g) + 6H2O (l). Can you help me figure out many moles of water will be produced when 16 moles of ethane are burned?

Question 2: Ammonia (NH3) is produced by the reaction of hydrogen gas with nitrogen gas: 3H2+N2→2NH3. A chemist reacts 2.00 mol H2 with excess N2. The reaction yields 0.80 mol NH3. Can you help me understand what is the percent yield of the reaction?

Question 3: Li3N(s)+3H2O(l)→NH3g)+3LiOH(l). If I need to make 120 g LiOH, how many grams of Li3N must I use to react with excess water?

Question 4: What is the volume of 2 moles of methane (CH4) when one mole of this gas occupies 22.4 L?

Question 5: In the hydrazine-nitrogen tetroxide rocket fuel reaction: 2N2H4+N2O4→3N2+4H2O, how many grams of N2H4 will be consumed by 23 g of N2O4?

Question 6: In the reaction of N2+3H2→2NH3, suppose we have 0.87 L of nitrogen. How many liters of hydrogen do we need for a complete reaction (assuming one mole of any gas occupies 22.4 L)?

Question 7: A reaction produces 4.93 L of oxygen, but was supposed to produce 1 mol of oxygen. What is the percent yield (assuming one mole of any gas occupies 22.4 L)?