Consider the following reaction representing the combustion of propane: \mathrm{CgH}_{4}+\mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} (a) Balance the equation. (b) How many moles of oxygen are required to burn 1 mol of

propane? (c) How many grams of oxygen are required to burn 100 g of propane? (d) At standard temperature and pressure, what volume of oxygen would be required to burn 100 g of propane? If air is 21 percent oxygen, what volume of air at STP would be required? (e) At STP, what volume of CO, would be produced when 100 8 of propane are burned?