Calculate ideal-gas temperature of a material

AI Thread Summary
The discussion focuses on calculating the ideal-gas temperature using constant-volume thermometers and the relationship between pressure and temperature. The equation used is θ(P) = 273.16(P/P_TP), where P_TP is the thermometer's pressure at the triple point. It is noted that as the constant volume increases, the triple point pressure decreases, leading to a limiting value as pressure approaches zero. The calculated ideal-gas temperature from the plot is 419.55K, while the book states it is 1.5356K, raising questions about the discrepancy. The suggestion is made to incorporate thermometer volume into the calculations for more accurate extrapolation to the ideal-gas temperature.
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Homework Statement
In the table below, a number in the top row represents the pressure of a gas in the bulb of a constant-volume gas thermometer (corrected for dead space, thermal expansion of bulb, etc) when the bulb is immersed in a water triple-point cell. The bottom row represents the corresponding readings of pressure when the bulb is surrounded by a material at a constant unknown temperature.

Calculate the ideal-gas temperature of this material to five significant figures.
Relevant Equations
Please see table and calculations in what follows.
Here is the table
1696312349432.png
As far as I can tell what we have here are four constant-volume thermometers (each column represents a thermometer). These thermometers work by having a certain constant volume of some specific gas in a bulb. We immerse the bulb in whatever temperature we would like to measure, and measure the pressure required to keep the volume constant.

Then we use the equation ##\theta(P)=273.16\frac{P}{P_{TP}}## where ##P_{TP}## is the pressure of the thermometer in question when immersed in the water triple-point cell.

For the four thermometers in this problem we have

1696312484909.png


Notice that for each successive thermometer, the triple point pressure is lower. This happens because the amount of constant volume is successively larger for each thermometer.

If we keep reducing the constant volume and measuring the pressure of the unknown material, we will reach some limiting value

$$\lim\limits_{P_{TP}\to 0} 237.16\cdot\frac{P}{P_{TP}}$$

Now, I don't see how to calculate this limit other than to extrapolate from the observed values.

If we plot the constant volume of each thermometer vs the empirical temperature using that thermometer then we get the following

1696312584474.png

The ideal-gas temperature would be wherever the plot intercepts the vertical axis, let's call it 419.55K.

Is this correct?

When I look at the answer at the end of the book I am reading, it says the answer is 1.5356K. This seems to be related to the ratio of pressures only, not the ratio times the triple point temperature in kelvin. That is,

1696313257045.png

Why is the book calling this the ideal-gas temperature? Or is it an error?

The book is "Heat and Thermodynamics", Seventh Edition, by Zemansky and Dittman, and the problem is 1.1 (Chapter 1, problem 1).
 
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I agree with your assessment.
 
Wrt the asymptote, it seems to me you need a formula which includes the thermometer volume, ##V_{th}##. If you can rearrange it in the form ##y=V_{th}x+\theta## and do a linear regression then you can extrapolate to ##V_{th}=0##.
 
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