Summary: In part A, we found out the gas pressure times the gas volume is a constant at the same temperature. This is Boyle’s law. In part B, we got the gas pressure and the gas temperature is in direct proportion at the same volume. This is Gay Lussac's law. Based on these two laws and Charles’s law, the chemists expand the ideal gas law. The ideal gas law describes the ideal gas’s pressure, volume, mole and temperature relationships. The ideal gas equation is PV = nRT. It is no ideal gas in the world, but there are four variables in this equation. So we can use this equation for real gas. Discussion/Conclusions: The relationship between the pressure and volume of a confined gas is inverse. Because when the volume got larger, the pressure got smaller. Based on my data, I got a function between the gas pressure and volume is y = -8.9505x + 102.51. We put 60.0mL into x then got y is equal -434.52kPa. In the same way, we put 0.20mL into x then got y is equal 100.72kPa. We assumed the mole and temperature are constants in part A experiment. From my answer to Question one,
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