Question

This is all in the context of a Gas Laws labratory involvingBoyle's Law and Amonton's Law:

For Boyle's Law the class used the Vernier pressure sensor todetermine the pressure of nine syringe readings, ranging from 60 to20 mL. With those values we multiplied the pressure by the Volume(total) for each reading and compared each to the averagecalculated K valule.

An example equation for a readings is as follows:

Volume syringe = 60mL, pressure (atm) = 1.206, Volume of smalltube (constant through the experiment, = 3.28),

Pressure (1.206atm) x Volume total (60+volume tube (3.28)) =64.444528.

Average value = 65.69823

(64.444528-65.69823)/65.69823 = -1.146

The -1.146 value is the change in percent from the calculatedvalue to the average.

For Amonton's Law, the apparatus was assembled to hold anErnlynmyer flask within a 1 L water bath that is gradually heatedto 80 degrees C. As the temperature increases, the class collectsthe pressure reading within the flask in incriments of 2 degrees soa graph can be contructed with pressure on its x axis andtemperature on the y. Once these points are plotted, the graph canbe extrapolated to determine a calculated estimate as to whatabsolute zero should be.

The trendline equation determined was y=.00423189x +.9022160.

Solving for zero, the absolute zero temperature is-214.1411048.

1. Is it necessary to know the volume of the apparatus in thispart of the experiment? Why or why not?

2. Ideally, what should happen to the pressure of a gas if theKelvin temperature is doubled?

3. Which technique, extrapolation or interpolation, is morereliable and why?