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- Homework Statement
- A thermally insulated container is divided into ##2n+1## equal sections by ##2n## walls, each containing monoatomic ideal gas with the same pressure and temperature. The walls with odd numbers (from ##1## to ##2n-1##) are fixed and good heat conductors, the walls with even numbers (from ##2## to ##2n##) are thermally insulating and freely moving like pistons. Similarly the ##0^{\text{th}}## wall is thermally insulating and is moveable. This gas in the first section of the container is slowly being compressed by moving the ##0^{\text{th}}## wall. How does the temperature of the gas in this section change as a function of its volume? What can we say about the displacements of the freely moving walls?
- Relevant Equations
- ##TV^{\gamma -1}##, where ##\gamma## is heat capacity ratio.
IMO, this problem is really tricky. Here below is my attempt.
Let us take a perfectly insulated container and imagine dividing it with an alternating series of walls: those with an odd index are rigid and conduct heat, bringing the two adjacent compartments into thermal contact; those with an even index, including the ##0^{\text{th}}## we are pushing, are ideal adiabatic cylinders, i.e. they slide without friction maintaining the same pressure on both sides but not allowing heat to pass through.
The compartments are initially all identical, filled with the same monoatomic gas at temperature ##T_0## and volume ##V_{\text{initial}}##.
The conductive walls weld the compartments ##0##-##1, 2##-##3, \ldots , 2n-2##-##2n-1## in pairs: this results in ##n## "double blocks", while compartment ##2n## remains the only "single block". Since each block is enclosed by adiabatic pistons, the gas it contains obeys the polytropic process equation ##T V^{\gamma-1}= \text{constant}## with ##\gamma =5/3##; in addition, the pressure must remain the same in all compartments for the pistons not to gain acceleration. These two conditions force the volume of a double block to remain exactly twice that of the single block throughout the transformation: ##V_{\text{double}} : V_{\text{single}} = 2 : 1##.
Let us now suppose we slowly push ##0^{\text{th}}## piston, reducing its volume from ##V_{\text{initial}}## to ##V## (if we are compressing it, ##V < V_{\text{initial}}##). The overall volume of the gas changes from ##(2n+1) V_{\text{initial}}## to ##V_{\text{tot}} = 2n V_{\text{initial}} + V##. The ##0##-##1## block must preserve the ##2:1## ratio and therefore takes ##V_{01}=\dfrac{2(2n V_{\text{initial}} + V)}{2n+1}## at each instant. Applying the polytropic process equation to that block, we immediately obtain the temperature of the gas in compartment ##0##: $$T(V)=T_0 \left[\frac{(2n+1) V_{\text{initial}}}{2n V_{\text{initial}}+V}\right]^{2/3}.$$
This result shows that the longer the chain of pistons (##n## large), the slower the temperature rises: the work we exert on the first piston is redistributed over many blocks. In the case ##n \to \infty##, we would obtain ##T(V) \to T_0##.
I am very suspicious of this result. It is expressed as a function of unknown variables from the text, and I don't know if the train of thought is correct.
As for the displacements of the internal pistons, we denote ##\Delta V=V-V_{\text{initial}}## (##< 0## in compression) and let ##S## be the cross-section of the container. The piston of index ##2k \,\, (k=0,1, \ldots, n)## moves back by $$\Delta x_{2k}=\frac{V_{\text{initial}}-V}{S} \cdot \frac{2n+1-2k}{2n+1} \qquad \text{for} \quad k = 0, 1, \ldots, n.$$
Piston ##0## runs ##(V_{\text{initial}}-V)/S##, piston ##2n## just runs ##\dfrac{1}{2n+1} \cdot \dfrac{V_{\text{initial}}-V}{S}##, and between those extremes, the displacements decrease linearly: each internal piston always advances by a fixed amount less than the previous one.
Again, I am very suspicious of this result. It is expressed as a function of unknown variables from the text, and I don't know if the train of thought is correct.
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