A closed system in thermodynamics refers to a system that can exchange energy with its surroundings in the form of heat or work, but not matter. This means that while energy can flow into or out of the system, no mass is transferred across the system's boundaries.
In a closed system, the total energy of the system is conserved. This means that the sum of the internal energy, pressure-volume work, and heat added to or removed from the system is constant over time. The internal energy of the system is the sum of the kinetic and potential energies of all particles within the system.
The closed system can interact with its surroundings by exchanging heat and work. Heat transfer occurs when there is a temperature difference between the system and its surroundings, resulting in the flow of energy from the higher to the lower temperature region. Work transfer, on the other hand, occurs when there is a difference in pressure or a change in volume of the system.
The conservation of energy in a closed system can be stated as the first law of thermodynamics, which is an expression of the principle of energy conservation. It is given by the equation:
ΔU = Q - W
where ΔU is the change in internal energy of the system, Q is the heat added to the system, and W is the work done by the system.
Overall, a closed system in thermodynamics is a system that can exchange energy with its surroundings but not matter, and the total energy of the system is conserved through the exchange of heat and work.
Explain the close system in thermodynamic system
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