When answering the question, please explain the steps and the meaning, I'm really lost. Thank you!

Consider the following reaction representing the combustion of propane: C3H8+O2CO2+H2O (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 100g of propane? (d) At standard temperature and pressure, what volume of oxygen would be required to burn 100g of propane? If air is 21 percent oxygen, what volume of air at STP would be required? (e) At STP, what volume of CO2 would be produced when 100g of propane are burned