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Thermal Physics? Thermodynamics?

Fig.: Thermodynamics and related subjects.

In classical mechanics, the field of kinematics
describes moving objects using quantities such as length $s$, time $t$, velocity $v=\frac{{\rm d}s}{{\rm d}t}$ and acceleration $a=\frac{{\rm d}^2s}{{\rm d}t^2}$. Dynamics
is the part of classical mechanics which explains the causes of the motion of objects. It is here that mass $m$, momentum $p=mv$, force $F=ma$ and energy $E=Fs$ are introduced. Thermodynamics
takes this one step further by introducing temperature
as an additional quantity, heat
as an energy relating to temperature changes, and entropy
as a quality assigned to energy.

Within thermodynamics, we can distinguish classical thermodynamics
, which describes the behaviour of macroscopic objects and phenomena, from statistical mechanics
, which deals with microscopic interpretations of such macroscopic properties using statistical methods and models.

Fig.: Interatomic potentials.

The term thermal physics
is synonymous with thermodynamics in this wider sense, but emphasises the physical aspects of this interdisciplinary field. Thermodynamics is equally central to adjacent disciplines such as chemistry, mechanical engineering, and information theory. Engineering thermodynamics
is at the root of the discipline, which was first established as a theoretical foundation to understand the operation and efficiency of heat engines. Chemical thermodynamics
uses concepts such as equilibrium to predict how chemical reactions unfold. In recent decades, concepts from statistical thermodynamics, particularly entropy, have been applied to information theory
, leading to applications such as cryptography.

Fig.: Pressure as cumulative force from moving gas molecules.

The kinetic theory of gases
is at the crossover of the classical and statistical branches of thermodynamics. It considers the thermal movements of gas molecules to derive the pressure the gas exerts on the walls of a vessel. The higher the temperature of the gas, the higher the mobility of the gas molecules and thus the higher the force each molecule hitting a wall transfers to the wall. Since the thermal motion is randomly orientated, the forces from the particles cancel each other out and simply add up to a uniform pressure (force per surface area) on the walls surrounding the gas.

If the walls are static, the volume must remain constant and pressure builds up inside the vessel - a pressure cooker
or boiler. If the walls are flexible, they can expand until the forces acting from the inside and outside are balanced, i.e. the pressure remains constant but the volume expands - a hot-air balloon.

Thermodynamic states and state variables

Fig.: System, walls and surroundings.

Thermodynamics divides the world into the system
under study and its surroundings
. Both are separated by walls
. These terms are used conceptually and are not limited to any particular material or process; a "wall" can be as insubstantial as a foam bubble. Walls may or may not be permeable to transfers of various forms of energy and matter. Systems can be nested, e.g. we might consider the boiler inside a power station as a system and be concerned with the temperature and pressure inside it and the energy flows into and out of it, or we could treat the whole power station as a system and consider its relationship with its surroundings including the power grid and the atmosphere. It is therefore important to be clear about what the system is that is being investigated.

Fig.: State variables are constant over time in the absence of interaction.

A state
in thermodynamics is a complete description of a system in terms of physical quantities. The physical quantities are known as state variables
. State variables are either intensive
(uniform throughout the system, e.g. pressure or temperature) or extensive
(they add up throughout the system, e.g. mass, volume, number of atoms, internal energy, entropy). State variables do not change without external interaction with the system. Atoms in a gas move about, but the number of gas atoms inside a container doesn't change unless we interact with the system to let some atoms out.

Fig.: State variables are not independent of each other.

State variables depend on each other.
If you heat a pressure cooker, the pressure will increase along with the temperature. If you heat a balloon, the volume increases with temperature. Anything done to a system that changes its state is known in thermodynamics as a process

Thermodynamics often uses an engine cylinder containing a gas as a working medium as a metaphor for any interacting system. This is largely for historical reasons, but also because it is a simple model system where state variables and energy flows are relatively easy to determine. Consider a cylinder with a piston and a safety valve which will open if the pressure in the cylinder exceeds a certain level. If the piston is pushed into the cylinder, the gas will contract (i.e. its volume decreases), but if we don't overdo it, the valve will remain closed. One state variable (volume) responds to a change in another (pressure); other state variables (amount of atoms, temperature) are unaffected. Suppose we put a burner under the cylinder next. Now the temperature increases. If we don't let the piston go, the pressure increases further until the safety valve opens. Now gas is released until the pressure comes down to safe levels. Again, one state variable (amount of atoms) responds to a change in another (temperature) while others (pressure, volume) are unaffected. One could argue that the volume changes because the gas spills over into the space outside, but we've defined the cylinder as our system, so the atoms have escaped into the surroundings in this process.

Fig.: State changes are path independent.

Sometimes, the term state function is used to stress the fact that a state variable depends on other state variables. The dependency works boths ways, though, so it's a matter of taste which state variable is treated as the (dependent) state function and which ones are treated as (independent) state variables. For example, in step 1 of the experiment, we could say that the volume is a state function of pressure, amount and temperature: $V(p,n,T)$.

Instead of applying pressure first and heating later (path A), we could have gone the other way to reach the same end result. Alternatively (path B), by heating the original cylinder (initial state), the gas will expand, pushing the piston out. By acting against that expansion and pushing the piston in, we end up with the same final state with gas being ejected from the safety valve.

Exercise. The ideal gas law (see below) expresses pressure as a function of other state variables, $$p=\frac{nRT}{V}\qquad.$$ Show that the end result is the same whether the gas is heated first and then compressed (path 1) or the other way around (path 2) by applying Schwarz's theorem.

The order of changes of state variables doesn't change the end result, in other words processes (state changes) are path independent. Mathemtically speaking, we can say that if a state variable $x$ depends on two other state variables $y$ and $z$, then the mixed second derivative is commutative: $$\frac{\partial^2x}{\partial y\partial z}=\frac{\partial^2x}{\partial z\partial y}\qquad.$$ This is known as Schwarz's theorem in maths and applies to all functions of several variables whose mixed second derivatives are continuous.

Thermodynamic equilibrium

Fig.: Equilibrium - state changes aren't instantaneous.

When a state variable is being changed in practice, it doesn't immediately change uniformly throughout the system. For example, the water in a pot on a stove will at first be hotter at the bottom, near the heat source. The system isn't in a defined state because the intensive state variables aren't uniform throughout the system. It takes a while for the system to reach equilibrium

In thermodynamic equilibrium, all state variables are constant over time and uniform throughout the system.

Exercise. A pizza is cooked at $T_0=\mathrm{220^{\circ}C}$. At $t_0=\mathrm{0\,min}$, it is removed from the oven and put on the table at an ambient temperature of $T_{\infty}=\mathrm{20^{\circ}C}$. At $t_1=\mathrm{3\,min}$, it has cooled to an edible $T_1=\mathrm{70^{\circ}C}$.

Fig.: Pizza.
Image: ElfQrin via Wikimedia

What is the relaxation time of the pizza?

When will it have cooled to $T_2=\mathrm{30^{\circ}C}$?

The process of reaching equilibrium after an external interaction with the system is called equilibration
or relaxation. It usually follows an exponential time dependence of the type $$x=x_0\exp{\left(-\frac{t}{\tau}\right)}$$ where $x$ is a state variable, $x_0$ its initial value, $t$ is elapsing time and $\tau$ is the relaxation time, a time constant describing how fast the system relaxes back to equilibrium. Of course, the exponential function is asymptotic, so equilibrium is approached but never really reached.

The ideal gas

As we have seen, the state variables depend on each other. What exactly this dependence is depends on the medium. We need a model for the medium that allows us to describe mathematically how the different state variables are linked. This is known as an equation of state

Exercise. Which of the state variables in the ideal gas law are intensive?

Just as classical thermodynamics models the world in terms of piston cylinders, it uses a simple model for the medium, the ideal gas
. Of course, as with any model, reality will deviate from it sooner or later, and a number of refinements have been proposed to deal with deviations from the simple assumptions the model is based on. The ideal gas is a gas without interactions between the individual gas atoms, and temperature and pressure are proportional to each other with a uniform constant of proportionality. This produces the ideal gas law: $$pV=nRT$$ where $R$ is the gas constant, $R=N_Ak_B$, the product of Avogadro's and Boltzmann's constants. Its value is 8.314 J/(K mol).

Now that the basic terms are defined, we can consider thermodynamic equilibrium further and develop the laws of thermodynamics.