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The internal energy of a thermodynamic system is the energy of the system as a state function, measured as the quantity of energy necessary to bring the system from its standard internal state to its present internal state of interest, accounting for the gains and losses of energy due to changes in its internal state, including such quantities ...
A reaction or process in which heat is transferred to a system from its surroundings is endothermic. The first law of thermodynamics states that the energy of the universe is constant. The change in the internal energy of a system is the sum of the heat transferred and the work done.
An energy form inherent in every system is the internal energy, which arises from the molecular state of motion of matter. The symbol U is used for the internal energy and the unit of measurement is the joules (J).
The first law of thermodynamics is given as \(\Delta U = Q - W\), where \(\Delta U\) is the change in internal energy of a system, \(Q\) is the net heat transfer (the sum of all heat transfer into and out of the system), and \(W\) is the net work done (the sum of all work done on or by the system).
The internal energy of a system is made up of many components, any or all of which may be increased when you add heat to the system or do work on it. If the system is a gas, for example, the internal energy includes the translational, vibrational and rotational kinetic energies of the molecules.
Internal Energy. The internal energy \(E_{int}\) of a thermodynamic system is, by definition, the sum of the mechanical energies of all the molecules or entities in the system.
Internal energy (internal heat energy) of a system is the sum of all the individual kinetic energies of motion and energies of interaction (potential energies) of the particles in the system. Internal energy can be transformed to do work and produce heat.
