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The entropy of an ideal monatomic gas is \((3 / 2) N k_{B} \ln E+\) \(N k_{\mathrm{B}} \ln V-N k_{\mathrm{B}} \ln N,\) to within an additive constant. Show that this implies the correct relationship between internal energy \(E\) and temperature.

Short Answer

Expert verified
The relationship between internal energy \(E\) and temperature of an ideal monatomic gas is \(E =(3/2)N k_B T\).

Step by step solution

01

Express entropy in terms of temperature.

The entropy \(S\) for an ideal gas is given as \((3/2)N k_B \ln E+N k_B \ln V-N k_B\ln N\). In order to find the relationship between \(E\) and \(T\), we first express entropy in terms of temperature. We use the definition of temperature as \(1/T = \partial S / \partial E\) where \(\partial S\) is the change in entropy, \(\partial E\) is the change in internal energy \(E\) and \(T\) is the temperature. This forms the basis to obtain an expression for temperature in relation to the internal energy.
02

Differentiate the entropy expression with respect to \(E\)

Now that the entropy is expressed in terms of temperature, we need to derive it with respect to \(E\). Using the properties of logarithmic differentiation, the derivation of \(S\) with respect to \(E\) gives \((3/2)N k_B / E\). This is substitution into the definition of temperature.
03

Solve for internal energy \(E\)

Substitute the derived expression for \(\partial S / \partial E\) into the definition of temperature. This gives \(1/T = (3/2)N k_B / E\). Thus, the internal energy \(E\) is equal to \(E =(3/2)N k_B T\) in terms of temperature. This relationship corresponds to the energy of an ideal monatomic gas.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Relationship Between Internal Energy and Temperature
Internal energy is a fundamental concept in thermodynamics; it represents the total kinetic and potential energy of molecules in a substance. For an ideal monatomic gas, this internal energy is directly related to temperature, a measure of the average kinetic energy of its particles.

In a monatomic gas, which consists of single atoms, potential energy interactions between atoms are negligible, and thus the internal energy depends solely on kinetic energy. This energy is proportional to the temperature of the gas and is described by the equation \(E = (3/2)Nk_BT\), where \(E\) is the internal energy, \(N\) is the number of particles, \(k_B\) is Boltzmann's constant, and \(T\) is the temperature in Kelvin. The factor \(3/2\) arises from the degrees of freedom available to a monatomic particle in three-dimensional space (translational motion along x, y, and z axes).

The relationship holds because as the temperature increases, the particles move faster and the overall kinetic energy of the system increases. This linear relationship between internal energy and temperature is a cornerstone of classical thermodynamics and is essential in understanding the behaviour of ideal gases.
Logarithmic Differentiation
Logarithmic differentiation is a mathematical technique used to differentiate functions that can be difficult to handle using standard rules of differentiation. It is particularly useful when dealing with functions involving products, quotients, or powers that depend on the variable.

To apply logarithmic differentiation, take the natural logarithm (ln) of both sides of an equation, and then use the property of logarithms to simplify the expression. This often turns multiplications into additions and powers into multiplications by their exponents. Once simplified, differentiate both sides with respect to the variable.

Example in Thermodynamics

In thermodynamics, logarithmic differentiation can be employed to solve for the change in entropy \((\text{d}S)\) with respect to internal energy \((\text{d}E)\). The entropy expression can involve natural logarithms, as it does for an ideal monatomic gas. By differentiating \(S\) with respect to \(E\), you obtain a relation that can be used to express the temperature in terms of \((E)\), which is crucial for understanding thermodynamic processes within the gas.
Definition of Temperature in Thermodynamics
The definition of temperature in thermodynamics is a bit more nuanced than the everyday concept of how hot or cold something feels. In thermodynamics, temperature is defined as a measure of the average kinetic energy of the particles in a system.

More formally, temperature is related to the direction of heat flow between systems in contact: heat flows from the system with higher temperature to the system with lower temperature. In terms of entropy \(S\) and internal energy \(E\), temperature \(T\) is defined through a partial differential relationship, where \(1/T\) is the change in entropy with respect to the change in internal energy at constant volume and the number of particles: \(1/T = (\text{\textpartial}S / \text{\textpartial}E)_{V,N}\).

This strict thermodynamic definition implies that on a microscopic level, temperature influences not just the speed at which particles are moving, but also the rate at which energy states are occupied, which has critical implications for the study of entropy and the laws governing heat, work, and energy transformations.

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Most popular questions from this chapter

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The exact probabilities of equation \((9-9)\) rest on the claim that the number of ways of adding \(N\) distinct nonnegative integers to give a total of \(M\) is \((M+N-1) !\) \([M !(N-1) !]\). One way to prove it involves the following trick. It represents two ways that \(N\) distinct integers can add to \(M-9\) and 5 , respectively, in this special case. $$ \begin{array}{c|cccccccccccccc} \hline \text { 1 } & \text { X } & \text { X } & \text { X } & \text { I } & \text { I } & \text { X } & \text { I } & \text { I } & \text { I } & \text { I } & \text { X } & \text { I } & \text { I } \\ \hline 2 & \text { I } & \text { X } & \text { X } & \text { I } & \text { I } & \text { I } & \text { I } & \text { X } & \text { I } & \text { I } & \text { I } & \text { X } & \text { X } \\ \hline \end{array} $$ The X's represent the total of the integers, \(M\) - each row has \(5 .\) The I's represent "dividers" between the distinct integers, of which there will of course be \(N-\) I -each row has 8 . The first row says that \(n_{1}\) is 3 (three \(X\) 's before the divider between it and \(n_{2}\) ). \(n_{2}\) is 0 (no \(X\) 's between its left divider with \(n_{1}\) and its right divider with \(\left.n_{3}\right), n_{3}\) is \(1, n_{4}\) through \(n_{6}\) are \(0, n_{2}\) is \(1,\) and \(n_{8}\) and \(n_{9}\) are 0\. The second row says that \(n_{2}\) is \(2, n_{6}\) is \(1, n_{9}\) is \(2,\) and all other \(n\) are 0 . Further rows could account for all possible ways that the integers can add to \(M\). Argue that. properly applied, the binomial coefficient (discussed in Appendix J) can be invoked to give the correct total number of ways for any \(N\) and \(M\).

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