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)
-6	24.6
9	25.7
35	28.1
38	28.4
65	31.0
71	31.5
81	32.4
89	33.1
95	33.8
99	34.0