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The internal energy (U) can be calculated by adding the heat transferred (Q) to the work done (W) on a system. This equation is based on the first law of thermodynamics which states that energy cannot be created or destroyed, only transferred or converted from one form to another.
The internal energy is a sum of the heat and work done on a system. Heat is the transfer of energy due to a temperature difference, while work is the transfer of energy due to a force acting over a distance. Together, they contribute to the change in internal energy of a system.
Yes, it is possible for internal energy to be negative. This would occur if the system loses heat or does work on the surroundings, resulting in a decrease in its internal energy.
The SI unit for internal energy is joules (J). However, other units such as calories (cal) or electron volts (eV) may also be used depending on the system being studied.
Temperature is a measure of the average kinetic energy of particles in a system. As temperature increases, the particles have more energy and therefore the internal energy of the system also increases. However, the internal energy also depends on other factors such as pressure and volume, which can affect the temperature as well.
