Thermodynamics
Heat
The particles that make up all matter are in a state of perpetual motion. This internal kinetic energy manifests itself as the form of energy called heat. The study of heat is thermodynamics. All mater is made up of moving particles; therefore, all mater has heat.
Heat is a form of energy and is measure in terms of the amount of work done. In the metric system, there are two units commonly used. Physicists most often use the calorie, the amount of heat needed to raise the temperature of 1 gram of water by 1 Celsius A kilocalorie, or Calorie, is the amount of heat required to raise the temperature of a kilogram of water 1 Celsius. The Calorie with a capital C is the one used to measure the energy content of foods. In the fps system, a British thermal unit (Btu) is the amount of heat required to raise the temperature of 1 pound of water 1 Fahrenheit.
Temperature is not the same as heat. Temperature is a measure of the average kinetic energy of the particles of an object, while heat is a measure of the total kinetic energy. The Kelvin, or absolute, scale of temperature is based on the idea that there is a temperature at which all particle motion ceases. This is temperature is called absolute zero and has been calculated to be 273.16 degrees below zero Celsius.
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Conservation of Mass-Energy
Energy can neither be created nor destroyed but only changed in type. This law is a generalization of the first law of thermodynamics, which states that when heat is transformed into other kinds of energy, the total energy remains constant.
In nuclear reactions, however, mass is converted to energy. Since matter can be considered a third form of energy, this principle is often called the law of conservation of mass-energy.
Heat and Work
To get work out of randomly moving particles, you must induce them to move predominantly in one direction or to supply energy in a single direction. Heat is transferred from any body of a higher temperature to a body of a lower temperature. The efficiency of a heat engine is proportional to this temperature difference. As heat is transferred, the difference is reduced. The fraction of the energy that flows into the cooler body becomes less available for transformation into work even though the total amount of energy is unchanged.
The statement that heat can never travel from a colder to a hotter body by any continuous, self-sustaining process is the second law of thermodynamics. That portion or quantity of energy that is lost as nonuseful heat is measured by entropy. Since heat in useful form is a result of particles in one place moving faster than particles somewhere else (that is, the first place is hotter than the second), entropy is also measure of disorder. The moving particles are statistically less ordered when the temperatures at both places are the same than when the temperatures are different. As a result, another version of the second law of thermodynamics is “Entropy (disorder) tends to increase.”