Polytropic processes

A polytropic process is described by the formula , where . The table below shows the association of different pV curves for ideal gases with the corresponding thermodynamic processes:

Question

Why is the projection (the curve obtained by representing the process in  space on the  plane ) an adiabat when and why is a constant when ?

Answer

From eq44 and eq46, and for an ideal gas. For adiabatic processes, and hence, . Furthermore, . Since , . So,


which rearranges to , where .

For the second why, . If , .

 

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Line integral

A line integral is the integral of a multi-variable function along a curve. Line integrals can be categorised into scalar line integrals and vector line integrals. They are usually evaluated using parametric equations, which are then reduced to one or more scalar integrals.

Scalar line integrals

Let’s begin with scalar line integrals. A scalar function of two variables is represented geometrically by a surface on a three-dimensional graph (see diagram above). Consider two points, A and B, on the surface. There are infinite ways to move along the surface between these two points. For simplicity, we have indicated two of these infinite paths using the red and pink curves, which can be projected onto the xy plane for better visualisation (see diagram below).

Due to the many paths available between the two points, the integral of between the points is not well defined. In other words, the integral is path-dependent. For a particular path, the integral of along this path, which is specified by one of the curves on the plane, is called a line integral.

Geometrically, the result is the area of the ‘curtain’ extending from that path, between and on the xy plane, to the curve on the surface (see diagram above), i.e.:

where denotes ‘curve’, which is the specified path linking the two points on the xy plane, and is the infinitesimal change in arc length along the curve.

Since the specific path is also a function of and , we convert and into parametric equations consisting of a single parameter and carry out the integration analytically (see 3rd Q&A below for an example).

 

Question

What if the two points, A and B, are the same?

Answer

In the scenario where the two points are the same, the infinite paths from to  are infinite loops. Similarly, integrating the function via different loops may give different results. Each line integral in this case is represented by:

where the circle on the integral sign denotes a loop or a cyclic process.

 

Vector line integrals

Let’s now look at vector line integrals, an example of which is the work done by a vector field (see diagram above). For instance, the work done by a variable force on a charged particle moving along some path in an electric field is

As mentioned in the opening paragraph, such a line integral is evaluated by converting it into one or more scalar integrals. We write and in terms of their two-dimensional Cartesian components:

which can then be evaluated when is specified.

 

Question

What is the difference between a scalar field and a vector field?

Answer

A scalar field, expressed by a scalar function , associates a scalar with each point in some region of space, while a vector field, expressed by a vector function  associates a vector with each point.

 

Line integral with respect to coordinates

Line integrals can also be carried out with respect to one of the function variables instead of with respect to the arc length, e.g. the scalar integral . The geometric interpretation of is the projection of on the plane (see above diagram). An example of such a line integral is the work done on an ideal gas in a reversible process:

If the path of the above integral is defined by introducing a constraint, e.g. when , where is a constant, we get a plane that intersects with the surface at a particular contour (see diagram below). A single curve, an isothermal curve, is then projected on the plane.

Consequently, the integral reduces to one involving a single variable:

Similarly, if the intersecting plane is or , the projection on the plane is a horizontal line (isobaric process) or a vertical line (isochoric process) respectively.

 

Line integral of differential forms

Line integrals are sometimes written in differential form. Consider the work done by a vector field on a particle moving along some path . We can write  and in terms of their components: and . So, eq92 becomes

Compared to the general differential equation of two independent variables of the form , the RHS of the third equality of the above equation is the line integral of a differential equation, which in this case is an inexact differential. In other words, .

In the case of an exact differential , its line integral is equal to the difference in values of the function at the final point and at the starting point:

This is known as the fundamental theorem of line integral. We call such a function, whose output is independent of the path taken to reach it, a state function.

 

Question

How do we proof the fundamental theorem of line integral?

Answer

Consider a function  with an exact differential of the form or

where  and .

To carry out the line integral between two points and , we convert the function into its parametric form, which is to let and  be some function of , i.e. . Correspondingly, we have and hence . So,

Using the definition of the chain rule for a multivariable function (see eq14b),

 

Finally, we have shown in a previous article that the change in internal energy of a system is path-independent for a system containing a perfect gas. We will show in the article on entropy that  is path-independent for any system. This makes an exact differential and , a state function. Thus, we can write

If the two points are the same, ,

Therefore, the change in internal energy in a cyclic process is zero: . In general, the line integral of any exact differential involved in a cyclic process is zero.

 

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Applications of the Joule-Thomson effect

Two significant applications of the Joule-Thomson effect involve the Hampson-Linde cycle and the vapour-compression cycle.

The Hampson-Linde cycle, also known as the ‘Linde refrigerator’ (see diagram below), employs the Joule-Thomson effect to liquefy gases.

The cycle is as follows:

    1. The gas is compressed to allow it to circulate throughout the system. This raises the temperature of the gas because the kinetic energy of the gas molecules increases as they collide with the moving wall.
    2. The gas cools as it passes through the heat exchanger and cools further when it expands through the Joule-Thomson orifice. The system is designed with specific pressures before and after the orifice to ensure the gas cools upon expansion, as described by the Joule-Thomson effect.
    3. The low pressure gas is routed to the heat exchanger, cooling the warmer incoming gas, before returning to the compression chamber.
    4. Warm replenishment gas for replacing any liquefied gas is mixed with the returning gas. The net temperature of the gas after mixing is lower than its temperature in step1. Steps 1 to 4 is repeated until the air is cool enough to condense into the compartment below the orifice.

The vapour-compression cycle is used in household refrigerators and air conditioning units.

The cycle is as follows:

    1. Compression: The refrigerant gas is compressed by the compressor, allowing it to circulate throughout the system. This is not an isenthalpic process because work is done on the gas, which increases both the pressure and temperature of the refrigerant.
    2. Condensation: The hot, high-pressure refrigerant gas then passes through the condenser coils, usually located on the back or bottom of the appliance. As it cools, it condenses into a high-pressure liquid.
    3. Expansion: The flow of the high-pressure liquid refrigerant through an expansion valve, known as the Joule-Thomson orifice, can be modelled using the Joule-Thomson experiment. This causes the refrigerant’s pressure to drop, resulting in a mixture of liquid and vapour. The refrigerant is carefully selected based on its inversion temperature to ensure it cools upon expansion, as described by the Joule-Thomson effect.
    4. Evaporation: The low-pressure refrigerant then enters the evaporator coils (inside the refrigerator or air handler of an air conditioning unit). Here, it absorbs heat from the surrounding environment, which allows it to fully evaporate into a gas. This process cools down the air inside the refrigerator or the room.
    5. Cycle repeats: The refrigerant gas is then drawn back into the compressor to repeat the cycle. The desired temperature of the room or the interior of the refrigerator is monitored by a thermostat, which then signals the appropriate compression pressure to apply for subsequent cycles.

The desired temperature of the room or the interior of the refrigerator is monitored by a thermostat, which then signals the appropriate compression pressure to apply for subsequent cycles.

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The Joule-Thomson experiment

The Joule-Thomson experiment, an improved version of the Joule experiment, was conducted by James Joule and William Thomson in 1852 to study the thermodynamic properties of a gas expanding into a vacuum.

The experiment involves a system that is adiabatically insulated from its surroundings (see diagram above). The system consists of a double-piston cylinder that is separated into two compartments by a rigid porous plug. Constant pressures and , where , are applied to the left piston and the right piston respectively. As a result, the gas in the left compartment is slowly throttled irreversibly to the right compartment. Assuming that pressure is well defined in each compartment,  and . The total work done on the system is

According to the first law of thermodynamics for the entire system,

So,  or . If there is a change in temperature of the system, the experiment measures the change in gas temperature with the change in gas pressure at constant enthalpy, i.e. , which is defined as the Joule-Thomson coefficient :

The experiment is conducted multiple times by lowering  for a constant  and . A temperature-pressure plot of the results gives an isenthalpic curve (see diagram above). The gradient at a particular point of the curve is the Joule-Thomson coefficient with respect to and at that point. Since the change in pressure of the system is always negative, points on the curve that are associated with negative gradients correspond to the gas warming on expansion. Conversely, points on the curve that are associated with positive gradients correspond to the gas cooling on expansion. The point at which the gradient is zero is called the inversion point. Repeating the experiment by holding at new constant values and varying , we have multiple isenthapic curves:

The line connecting all inversion points is the inversion curve. The area on the left of the inversion curve is where cooling occurs for a gas when it expands into a vacuum, while the area on the right is where heating occurs. The temperature corresponding to the inversion curve at a given pressure is the inversion temperature of the gas at that pressure. If a vertical line is extended across the inversion curve at a particular pressure, it will intersect the curve at two points: an upper inversion temperature and a lower inversion temperature. Cooling upon expansion usually occurs when the temperature of the gas is between its upper and lower inversion temperatures prior to expansion. In other words, whether the expansion results in heating or cooling of the gas depends on the initial conditions and the properties of the gas. This phenomenon, known as the Joule-Thomson effect, is exploited in refrigeration processes.

Modern methods of measuring involve evaluating , which is known as the isothermal Joule-Thomson coefficient. To determine the relation between and , we refer to eq16, where . Using eq15, . Substituting eq46 and eq90 in this expression,

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The Joule experiment

The Joule experiment was an attempt by James Joule in 1843 to determine for a gas expanding into a vacuum.

The experiment involves a system that consists of a gas-filled compartment (A) and an evacuated compartment (B), both of which are immersed in a water bath (see diagram above). When the valve between the compartments is opened, the gas expands irreversibly from A to B, doing no work in the process. Assuming that no heat transfer occurs between the system and its surroundings, the first law of thermodynamics states that . If there is a change in temperature of the water bath, the experiment measures the change in gas temperature with the change in gas volume at constant internal energy, i.e. , which is defined as the Joule coefficient :

To determine , we refer to eq16, where . Using eq15, . Substituting eq44 and eq88 in this expression,

For an ideal gas is independent of the volume of the gas, i.e. , because there is no intermolecular forces between the molecules (see eq43a). We would therefore expect a non-zero  for a real gas. However, Joule’s experiment setup was too crude to measure a non-zero . An improved version of Joule’s experiment is the Joule-Thomson experiment.

 

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Reversible adiabatic processes

A reversible adiabatic process is a reversible thermodynamic process in which no heat or mass transfer occurs.

A reversible adiabatic expansion follows the path from B to C, while a reversible adiabatic compression follows the path from D to A. The curves describing the paths of adiabatic processes are called adiabats (see diagram above, where we have included two isotherms, AB and CD, for comparison).

A reversible adiabatic compression is carried out in a frictionless, insulated piston-cylinder device containing a gas (see diagram above). The gas undergoes infinitesimal steps of compression, resulting in an increase in the internal energy of the system and therefore the temperature of the system. Since no heat enters or leaves the system, and according to the first law of thermodynamics,

For an ideal gas, we have shown in a previous article that  and hence, work done on the ideal gas system for a reversible adiabatic compression is:

Substituting in eq84 and integrating throughout gives:

where we have assumed that the heat capacity of the ideal gas is independent of temperature over the temperature range of interest and therefore a constant.

Solving the above equation yields:

where .

Similarly, for an adiabatic expansion from B to C, we have

Equating eq85 and eq86,

Question

Show that internal energy of a system  containing a perfect gas is a state function using the diagram above where

AC: reversible isothermal process
AD: reversible adiabatic process
AB: reversible isobaric process
BC & CD: reversible isochoric processes

Answer

Consider the change in internal energy of a system containing one mole of ideal gas from point A to point C. The change can be brought about by three different paths, with the first being a reversible isothermal expansion (AC), where .

The second path involves a reversible adiabatic expansion (AD) followed by a reversible isochoric heating (DC). The changes in internal energy for paths AD and DC are:

The change in internal energy for path ADC is:

Since

The third path consists of a reversible isobaric expansion (AB) followed by a reversible isochoric cooling (BC). The change in internal energy for path AB is:

From a previous article, , and so

Substituting  and  in the above equation,

The change in internal energy for path BC is:

The change in internal energy for path ABC is:

Regardless of the path taken, the change in internal energy from point A to point C is the same. Therefore,  is a state function.

 

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Using Kirchhoff’s law to determine the standard enthalpy change of ionisation and electron gain

Ionisation energy of a species is defined as the energy for removing an electron from the ground state of the species. According to statistical thermodynamics, the ground state of a species is the electronic configuration of that species at absolute zero. If ionisation energy is defined at any other temperatures above absolute zero, there will be a range of ionisation energies for a particular species, as the electron then is removed from various excited states. Hence, ionisation energy is equal to the difference between the sum of enthalpies of formation of the ionised species and the electron at absolute zero, and the enthalpy of formation of the species at absolute zero.


Ionisation energies are presented in data tables using eq73 of the previous article, where  is the experimental temperature and is absolute zero.

Question

Calculate the first ionisation enthalpy of magnesium at 298.15K, given IE1 = 738 kJmol-1 and assuming the heat capacities at constant pressure of all species (including electron) are given by that of a perfect monoatomic gas of .

Answer



Using eq73,

 

With reference to the above example where the heat capacities at constant pressure of all species (including electron) are given by that of a perfect monoatomic gas of ,

where  is at absolute zero.

Similarly,

Therefore, the ionisation enthalpy of  is

Electron affinity is also a zero Kelvin process, as it is defined as the energy for the addition of an electron to a species in its ground state. Although an exothermic process, electron affinity (EA) is quoted in data tables as positive values, i.e.

Since the standard enthalpy change of electron gain of a species is the negative of the standard enthalpy change of ionisation of that species with an additional electron attached , i.e.

the enthalpy change of electron gain, assuming the heat capacities at constant pressure of all species (including electron) are given by that of a perfect monoatomic gas of , is determined by substituting eq83 in eq80 and eq81:

with the electron gain enthalpy of being:

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Using Kirchhoff’s law to determine the standard enthalpy change of reaction at 298K

The experimental result of the standard change in enthalpy for the combustion reaction is 281.93 kJmol-1 at 1200K. Find its standard change in enthalpy at 298.15K given:

According to Hess’ law,

At 1200K,

At 298.15K,

Subtracting eq71 from eq70,

Since all species in the reaction are in the gaseous state from 298.15K to 1200K, we can substitute eq66 in eq72,

Substituting eq68 in the 1st integral on the RHS of eq73,

Substituting the relevant values from the table above in eq73 and evaluating the integral (using the form expressed by eq74 for each integral in eq73),

and

Combining eq66 and eq69, for a reaction

 

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Kirchhoff’s law (thermodynamics)

Kirchhoff’s law describes the change in enthalpy of a reaction with respect to the change in temperature.

From eq37, the heat capacity at constant pressure is defined as the change of enthalpy with respect to the change in temperature at constant pressure, i.e. . In other words, is the gradient of the curve of enthalpy versus temperature at constant pressure.

for a perfect gas is independent of temperature and we get a straight line with a constant gradient when the enthalpy of a perfect gas at constant pressure is plotted against temperature,. However, for an ideal or real gas,  varies with temperature and eq37 becomes:

Integrating both sides of eq64 with respect to temperature,

Since is a state function, the line integral of eq65 gives

or, for the change in enthalpy of a reaction,

Eq66 (or eq66a) is known as Kirchhoff’s law, which is used to calculate the change in enthalpy of a substance (or a reaction) from to .

The computation of eq65 to eq66 (or eq66a) is only valid if the function  is continuous and differentiable within the limits of to . If eq66a has a temperature range that includes phase transitions, which result in points of discontinuity in (see diagram above), it has to be modified as follows:

To find an expression for , we use a power series to generate curves that fit experimental values of for different substances on versus temperature plots:

The set of constants , , , , etc. are specific to each chemical species and are the outcome of the polynomial regression. As the contribution of higher powers of to  is small, the expression is fairly well represented by:

 

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Equipartition theorem: Vibrational motion

The vibrational energy of a diatomic molecule consists of a kinetic energy component and a potential energy component:

In classical mechanics, the potential energy  is equal to the work done against a force in moving a body from the reference point, where , to the displacement . In other words,

According to Hooke’s law, the vibrating diatomic molecule experiences a restoring force that is proportional to the displacement between the two atoms relative to its equilibrium or undistorted length:

where is the force constant.

Substituting eq55 in eq54 and integrating yields

Substituting eq56 in eq53 gives

From the theory of conservation of energy, the average kinetic energy of the molecule undergoing simple harmonic vibrational motion equals to the average potential energy of that molecule (see diagram above), i.e. . Hence, for a system of molecules, the average vibration energy of a molecule is:

According to the equipartition theorem mentioned in an earlier article, each kinetic energy component of a molecule has an average energy of . Hence, a diatomic molecule has an average vibrational energy of (vibration is along one axis).

For a molecule with atoms, we can derive its total component of motion as follows:

The motion of an atom is described by three Cartesian coordinates: , and . The components of the motion of independently moving atoms are therefore . However, if these free atoms are bound together to form a molecule, the translational motion of the molecule has three degrees of freedom regardless of its structure (see this article). The molecule’s rotational motion has two degrees of freedom if it is linear and three degrees of freedom if it is non-linear. The remaining degrees of freedom are attributed to the vibrational motion of the -atom molecule. Therefore, we have:

 

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