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Propane, C3H8, is a hydrocarbon that is commonly used as a fuel.
(a) create balanced equation for the complete combustion of propane gas. (b) Calculate the volume of air at 25 °C and 1.00 atmosphere that is needed to completely combust 25.0 grams of propane. Assume that air is 21.0 percent O2 by volume. (Hint: we will see how to accomplish this calculation in a later chapter on gases—for now use the information that 1.00 L of air at 25 °C and 1.00 atm contains 0.275 g of O2 per liter.) (c) The heat of combustion of propane is −2,219.2 kJ/mol. Calculate the heat of formation, ΔHf ° of propane given that ΔHf ° of H2O(l) = −285.8 kJ/mol and ΔHf ° of CO2(g) = −393.5 kJ/mol. (d) Assuming that all of the heat released in burning 25.0 grams of propane is transferred to 4.00 kilograms of water, calculate the increase in temperature of the water.
 
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