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Internal energy
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Internal energy is the total kinetic and potential energy of all the molecules in a substance. It is the energy that is stored within a system due to the constant movement and interactions of its particles. Internal energy can be thermal energy, which is associated with the temperature of the system, or non-thermal energy, such as potential energy stored in chemical bonds or in the arrangement of atoms within a molecule. The internal energy of a system can change due to heat transfer or work done on or by the system.
Step-by-Step Bot
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Internal energy refers to the total energy contained within a system due to the motion and interactions of its particles. It includes the kinetic energy of the individual particles and the potential energy associated with their interactions.
The internal energy of a system can change due to various factors, such as the transfer of heat or work done on or by the system. The first law of thermodynamics states that the change in internal energy (ΔU) of a system is equal to the heat (Q) added to the system minus the work (W) done by the system:
ΔU = Q - W
If heat is added to the system, the internal energy increases, causing the particles to gain kinetic energy and their motion to become more vigorous. On the other hand, if work is done by the system (e.g., expansion of a gas against a piston), the energy is transferred out of the system, decreasing its internal energy.
It is important to note that internal energy is a state function, meaning it depends only on the current state of the system and not on the path taken to reach that state. In other words, the change in internal energy is independent of the process used to achieve it.