A coffee can (with a diameter of 6.0 inches, height of 6.5 inches, and a mass of 256 g) has a 1 cm diameter hole drilled in the bottom and a 1 cm diameter hole drilled in the side. The can is capped, inverted, and completely filled with natural gas (methane). Methane gas is lighter than air and will therefore escape from the top hole of the coffee can apparatus. At the instant that the methane gas begins to escape from the top hole, the gas is ignited with a match and the plume continues to burn as the methane escapes and mixes with air. As methane escapes from the top hole, air enters the can through the hole in the side, changing the composition of the gas inside. During the following two minutes, the flame changes in color from yellow to pale blue, and finally is small and barely visible. The gas mixture inside the can finally violently explodes sending the can bouncing off the lab bench. Assume the room is 1.00 atm and 23 oC
What is the net pressure-volume work after all of the methane has combusted with excess oxygen and after the CO2 and H2O produced has cooled back to 23 oC at 1 atm pressure (assume that the water remains in the air as gaseous water vapor for this calculation)?