suresh Understanding the Difference Between Heat and Work in Thermodynamics
When it comes to thermodynamics, the terms "heat" and "work" refer to two different forms of energy transfer. The key difference lies in the way energy is exchanged between a system and its surroundings.
Heat: Heat is the transfer of energy due to a temperature difference. It flows spontaneously from a substance at a higher temperature to one at a lower temperature. In thermodynamics, heat is denoted by the symbol Q.
Work: Work, on the other hand, is the transfer of energy due to a mechanical interaction. It is performed on or by a system and involves the application of force over a distance. In thermodynamics, work is denoted by the symbol W.
Despite their differences, heat and work are related through the First Law of Thermodynamics, which states that the total energy of a system remains constant. This law can be expressed as:
∆U = Q - W
Where ∆U is the change in the internal energy of the system, Q is the heat added to the system, and W is the work done by the system.
In conclusion, understanding the distinction between heat and work in thermodynamics is crucial for comprehending how energy is exchanged and transformed within a system.
Focus Keyword: Thermodynamics
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