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,
This is the end of the preview. Sign up
to
access the rest of the document.
This note was uploaded on 11/08/2011 for the course CHEM 117 CHEM 117 taught by Professor Joannagoodey during the Fall '10 term at Texas A&M.
 Fall '10
 JOANNAGOODEY

Click to edit the document details