A sample of argon gas is trapped in a long glass tube with a drop of mercury acting as a movable lid. The length (y, measured in cm) of this gas column (which of course is proportional to the volume of argon) is measure at various temperatures (x, in °C). The accuracy of the length measurement is 0.1 cm.

In 1787 Jacques Charles claimed that the volume of a gas held at constant pressure depended linearly on temperature:

V = V0(1 + T/T0)

where V0 is the volume of the gas at T=0 and we now interpret T = -T0 as the lowest possible temperature: absolute zero. (Note [contrary to fact] that if the argon remained in gaseous form at T=-T0, it would have V=0; which, of course, is impossible.)

In this experiment, volume is proportional to length so we can translate Charles' Law as:

L = L0(1 + T/T0)

where L0 is the length of the gas at T=0 etc. If we compare this law to the generic equation for a line, we find:

A = L0

B = L0/T0

so

T0 = A/B

  1. Fit this data to a linear relationship.
  2. Consider Charles' scientific claim of a linear relationship. Does this evidence (data) confirm or contradict this claim? Support your answer quantitatively.
  3. Properly report (sigfigs, error, units) the A and B parameters of the best-fit line.
  4. Use a spreadsheet to calculate T0, and properly report (sigfigs, error, units) the value.
  5. Self-document the spreadsheet and turn in a hardcopy of the page.
  6. Make a hardcopy plot of the data with best-fit curve.

X
(°C)
Y
(cm)
-624.6
925.7
3528.1
3828.4
6531.0
7131.5
8132.4
8933.1
9533.8
9934.0