I can derive three characteristics from the properties of gases. Compressibility, expandability, and the way gases occupy spaces more than liquids or solids in a taken form. A great example of this characteristic that we use to describe gas compressibility is the operation of a Porsche 911 sports car. A Porsche 911 sports car runs on an internal combustion engine (normally a V8/ but in this case I'm talking about a particular four-stroke), in which “compresses the gases” as I spoke. To operate, the engine piston extends out of the cylinder to create a vacuum that draws a mixture of oxygen and gasoline vapor into the engine cylinder compartment. Then, a few seconds later, the piston then rotates pushing back into the cylinder, compressing the gasoline/air type mixture to a new volume, relative to the volume it had when the piston rotated up its sleeve . The typical car has a compressibility ratio of 9 to 1, but this Porsche has a compressibility of about 7 to 1, which may mean that the gas-air mixture in the cylinder is compressed by a factor of 7. The second property What I would like to describe in gas is extensibility. Anyone who has entered a bathroom where many people have just taken a number 2 has experienced that the gases expand to fill their container, while the air in the disgusting bathroom fills with terrible smells of waste. Just like people smell at a Formula 1 race, the distinctive smell of C2H5OH ethanol spreads quickly across the race track as it makes its way through the cars and is also found on the pit stop track. Gases expand to fill their containers, so it is safe to say that the volume of a specific gas can be equal to its volume...... middle of paper...... which is shown in moles, so ideal the gas law should be used to solve for the volume or mass of bass involved in the reaction. For example, if I wanted to calculate the volume of NO2 produced by the combustion of 100 g of NH3, by reaction 4NH3 + 7O2 = 4NO2 + 6H2O. It could be solved by 100 g of NH3 multiplied by 1 mole of NH3/17.034 g of NH3 = 5.871 mole of NH3. But on the other hand, the chemical reaction is expressed in moles and not grams. The ideal gas law must therefore be used to determine the volume or mass of the gas involved in the reaction. Using the same example as before, if I wanted to continue the process: there is a molar ratio of NH3 to NO2 of 1 to 1 in the balanced combustion reaction, so 5.871 moles of NO2 will be formed. Use PV=nRT to solve for the volume at zero degrees (273.15 K) and 1 atm using the gas law constant R=008206 times atm times K-1 times mol -1.