Difference Between Thermochemistry and Thermodynamics | Thermochemistry vs Thermodynamics
1 6–16–1 Ch. 6 Thermochemistry The relationship between chemistry and energy Basic concept of thermodynamics Energy conversion: Energy: the capacity to. What is the difference between Thermochemistry and Thermodynamics? Thermochemistry describes the relationship of heat energy and. Concepts covered in this tutorial include the laws of thermodynamics, internal energy, heat, work, More rigorous Gibbs free energy / spontaneity relationship.
Thermodynamics is the branch of physical science that deals with the relations between heat and other forms of energy such as mechanical, electrical, or chemical energy.
It explains the relationship between all energy forms. The main idea of thermodynamics is the association of heat with work done by or on a system. There are several important terms in thermodynamics. A Thermodynamic System Enthalpy — the total energy content of a thermodynamic system.
Entropy — a thermodynamic expression explaining the inability of a thermodynamic system to convert its thermal energy into mechanical energy Thermodynamic state — the state of a system at a given temperature Thermodynamic equilibrium — the state of a thermodynamic system being in equilibrium with one or more other thermodynamic systems Work — the amount of energy that is transferred to the surrounding from a thermodynamic system.
Internal energy — the total energy of a thermodynamic system that is caused by the motion of molecules or atoms in that system. Thermodynamics includes a set of laws.Thermochemistry: Heat and Enthalpy
Second Law of Thermodynamics — Heat cannot flow from a colder location to a hotter area spontaneously. Third Law of Thermodynamics — As a system approach absolute zero, all processes cease and the entropy of the system becomes minimum. What is the Relationship Between Thermochemistry and Thermodynamics?
Thermochemistry is a branch of thermodynamics. What is the Difference Between Thermochemistry and Thermodynamics?
Thermochemistry vs Thermodynamics Thermochemistry is the study and measurement of heat energy associated with chemical reactions. The System and Surroundings One of the basic assumptions of thermodynamics is the idea that we can arbitrarily divide the universe into a system and its surroundings.
The boundary between the system and its surroundings can be as real as the walls of a beaker that separates a solution from the rest of the universe as in the figure below. Or it can be as imaginary as the set of points that divide the air just above the surface of a metal from the rest of the atmosphere as in the figure below.
Internal Energy One of the thermodynamic properties of a system is its internal energy, E, which is the sum of the kinetic and potential energies of the particles that form the system. The internal energy of a system can be understood by examining the simplest possible system: Because the particles in an ideal gas do not interact, this system has no potential energy.
The internal energy of an ideal gas is therefore the sum of the kinetic energies of the particles in the gas. The kinetic molecular theory assumes that the temperature of a gas is directly proportional to the average kinetic energy of its particles, as shown in the figure below.
The internal energy of an ideal gas is therefore directly proportional to the temperature of the gas. The internal energy of systems that are more complex than an ideal gas can't be measured directly. But the internal energy of the system is still proportional to its temperature.
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We can therefore monitor changes in the internal energy of a system by watching what happens to the temperature of the system. Whenever the temperature of the system increases we can conclude that the internal energy of the system has also increased.
Difference Between Thermochemistry and Thermodynamics
Assume, for the moment, that a thermometer immersed in a beaker of water on a hot plate reads This measurement can only describe the state of the system at that moment in time. It can't tell us whether the water was heated directly from room temperature to Temperature is therefore a state function.
It depends only on the state of the system at any moment in time, not the path used to get the system to that state. Because the internal energy of the system is proportional to its temperature, internal energy is also a state function. Any change in the internal energy of the system is equal to the difference between its initial and final values.
Energy can be transferred from the system to its surroundings, or vice versa, but it can't be created or destroyed.
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First Law of Thermodynamics: It says that the change in the internal energy of a system is equal to the sum of the heat gained or lost by the system and the work done by or on the system. When the hot plate is turned on, the system gains heat from its surroundings.
As a result, both the temperature and the internal energy of the system increase, and E is positive. When the hot plate is turned off, the water loses heat to its surroundings as it cools to room temperature, and E is negative. The relationship between internal energy and work can be understood by considering another concrete example: When work is done on this system by driving an electric current through the tungsten wire, the system becomes hotter and E is therefore positive.