Hi Everyone, first semester Physics student here and we are working on a tough lab this week, having to do with Boyle's Law...argghh!!! Anyways, here is my problem, and trying to work through it to obtain the correct answer...but it is stumping me!! The question as follows: 1. Suppose data was collected for a sample of 3.oo moles of the ideal gas represented by the Pressure versus Volume -1 graph below. What is the Kelvin temperature of the gas? the graph has P (pressure) for the Y axis, and 1/V for the x axis. The slope =45.6 atm L and is at an approximate 45 degree angle (straight line) on the graph. Any thoughts? I am trying to use the equation of P=nRT/V=constant/V to solve this, but am not sure where/how to start. P=total pressure of the gas V=Volume of the gas n=# of moles of gas T absolute temperature og gas in Kelvin It is given that R=8.314 J/mol and K=0.0821 atm liter/mol K And here is a real tough one... 2. 2.00 moles of an ideal gas at -50 degrees Celsius has a volum of 1.00 liter. What is the pressure (in atm) in the container?? I can't find the proper equation/setup for this one and am totaly lost here...these two problems are just evil!!! Please help, if you can!! Thanks!!