The study of thermodynamics is the branch of physics that studies and describes the thermodynamic transformations induced by heat and work in a thermodynamic system. These transformations are the result of processes that involve changes in the state variables of temperature and energy at the macrosopic level.
Classical thermodynamics is based on the concept of a macroscopic system, that is, a portion of mass physically or conceptually separated from the external environment, which is often assumed for convenience that it is not disturbed by the exchange of energy with the system.
The state of a macroscopic system that is in equilibrium conditions is specified by quantities called thermodynamic variables or state functions such as temperature, pressure, volume, and chemical composition. The main notations in chemical thermodynamics have been established by the International Union of Pure and Applied Chemistry.
However, there is a branch of thermodynamics, called non-equilibrium thermodynamics that studies thermodynamic processes characterized by the inability to achieve stable equilibrium conditions.
What Are the Laws of Thermodynamics?
The principles of thermodynamics were enunciated during the nineteenth century and regulate thermodynamic transformations, their progress, their limits. They are real axioms, unproven and unprovable, based on experience, on which the entire theory of thermodynamics is based.
We can distinguish three basic principles, plus a "zero" principle that defines temperature and is implicit in the other three.
Zero Law of Thermodynamics
When two interacting systems are in thermal equilibrium, they share some properties, which can be measured, giving them a precise numerical value. As a result, when two systems are in thermal equilibrium with a third, they are in equilibrium with each other and the shared property is temperature. The zero principle of thermodynamics simply says that if a body "A" is in thermal equilibrium with a body "B" and "B" is in thermal equilibrium with a body "C", then "A" and "C" are in thermal equilibrium equilibrium between them.
This principle explains the fact that two bodies at different temperatures, between which heat is exchanged (even if this concept is not present in the zero principle) end up reaching the same temperature.
In the kinetic zero formulation principle of thermodynamics is a tendency to reach a common average kinetic energy of the atoms and molecules of the bodies between which heat exchange leads: on average, as a result of collisions of the body's particles warmer, on average, faster, with colder body particles, on average slower, there will be energy going from the first to the second, tending to equal temperatures. The efficiency of energy exchange determines specific heats of the elements involved.
First Law of Thermodynamics
When a body is placed in contact with a relatively colder body, a transformation takes place that leads to a state of equilibrium in which the temperatures of the two bodies are equal, enhancing a transfer of energy between the warm body to the cold body.
To explain this phenomenon, eighteenth-century scientists assumed that a substance, present in greater amounts in the warmer body, passed into the colder body.
This hypothetical substance, called caloric, was thought of as a fluid capable of moving through mass improperly called matter. The first principle of thermodynamics identifies heat as a form of energy that can be converted into mechanical work and stored, but is not a material substance.
Heat, originally measured in calories, and work or energy, measured in joules, were shown experimentally to be actually equivalent. Each calorie is equivalent to approximately 4,186 joules.
The first principle is therefore a principle of conservation of energy. In every heat engine or heat engine, a certain amount of energy is transformed into work: there can be no machine that produces work without consuming energy. A similar machine, if it existed, would in fact produce the so-called perpetual motion of the first kind.
The first principle is traditionally stated as:
The variation of the internal energy of a closed thermodynamic system is equal to the difference between the heat supplied to the system and the work done by the system in the environment.
The corresponding mathematical formulation is expressed as:
ΔU = Q - L
where U is the internal energy of the system, Q is the heat supplied to the system and L is the work done by the system.
Internal energy means the sum of the kinetic energies and the interaction of the different particles in a system. Q is the heat exchanged between the environment and the system (positive if it is supplied to the system, negative if it is transferred by the system) and L is the work done (positive if the system does it in the environment, negative if the environment does it in the system).
The sign convention is influenced by the link with the study of heat engines, in which heat is (partially) transformed into work.
The alternative and equivalent formulations of the first principle are:
- For an open system, qw =? E where? E is assigned to the variation of the total energy, which is nothing more than the sum of the changes in the internal energy, the kinetic energy and the potential energy that this system possesses is. We see that for a closed system the kinetic and potential energy variations are zero and, therefore, we refer to the previous relationship.
- For a thermodynamic cycle, q = w, since the total variation of energy is zero, the system has, at the end of each cycle, again under the same starting conditions.
Second Law of Thermodynamics
There are several statements of the second principle, all equivalent, and each of the formulations emphasizes a particular aspect. It states that "it is impossible to carry out a cyclic machine that only results in the transfer of heat from a cold body to a warm one" (Clausius statement) or, equivalently, that "it is impossible to carry out a transformation whose result is only that of converting the heat extracted from a single source into mechanical work "(Kelvin's statement).
This last limitation denies the possibility of performing the so-called perpetual motion of the second species. L 'entropy the total of an isolated system remains unchanged when a reversible transformation takes place and increases when an irreversible transformation takes place.
Third Law of Thermodynamics
It is closely related to the latter and, in some cases, is considered a consequence of the latter. It can be stated by saying that "it is impossible to reach absolute zero with a finite number of transformations" and provides a precise definition of the quantity called entropy.
It also states that the entropy for a perfectly crystalline solid, at a temperature of 0 kelvin is equal to 0. It is easy to explain this statement through molecular thermodynamics: a perfectly crystalline solid is composed of a single complex (They are all ways of organize the molecules, if the molecules are all the same, regardless of the way they are arranged, macroscopically the crystal is always the same) and, being 0 kelvin, the energy of vibration, translation and rotation of the particles that compose is nothing, therefore, of Boltzmann's law S = k ln (1) = 0 where 1 are the complexes (in this case only one).
History of Thermodynamics
It was Sadi Carnot, in 1824, the first to show that work can be obtained from the exchange of heat between two sources at different temperatures. Through Carnot's theorem and Carnot's ideal machine (based on the Carnot cycle) he quantified this work and introduced the concept of thermodynamic efficiency.
In 1848 Lord Kelvin, using the Carnot machine, introduced the concept of effective thermodynamic temperature and is responsible for a statement of the second principle of thermodynamics.
In 1850 James Prescott Joule demonstrated the equality of the two forms of energy (then it was believed that the caloric liquid still existed).
Having arrived at this, the problem was raised that, if it were possible to obtain the total heat of work, it would not have been possible to obtain the inverse. This result also landed Clausius who in 1855 presented his inequality to recognize reversible processes of the irreversible and state of the entropy function.
In 1876 Willard Gibbs published the treatise "On the equilibrium of heterogeneous substances" (On the equilibrium of heterogeneous substances) which showed how a thermodynamic process could be represented graphically and how to study in this way energy, entropy, volume, temperature and pressure could foresee the eventual spontaneity of the process under consideration.
The case of thermodynamics is emblematic in history and in 'the epistemology of science: it is one of those cases in which practice has pioneered the theory itself: the first is designed for the steam engine, then its theoretical functioning was systematized through its basic principles.
What Is Chemical Thermodynamics?
Chemical thermodynamics is the study of the interrelationship between heat and work with chemical reactions or with physical changes of state within the confines of thermodynamic laws.