Final answer:
An example of a violation of the First Law of Thermodynamics would be if the internal energy of an insulated, closed system changed without any energy transfer. This law states that energy in a closed system is conserved. Scenarios contradicting this, such as a box heating up spontaneously, would violate the First Law.
Step-by-step explanation:
The First Law of Thermodynamics, which is also known as the Law of Conservation of Energy, states that the energy of a closed system is conserved. If we have an empty, well-insulated cardboard box where no heat or electric current can pass through the walls, it means that the system is isolated and no heat has been exchanged with the surroundings (q = 0).
A scenario that necessarily violates the First Law of Thermodynamics would be one where the internal energy of the box changes without any energy entering or leaving the system. For instance, if the box suddenly became hotter or started moving without any energy input, this would contradict the law that energy cannot be created or destroyed within the closed system.
In contrast, the Second Law of Thermodynamics deals with the direction of thermodynamic processes and explains why certain processes do not occur, like heat spontaneously flowing from a cold object to a hot one without external work. While the First Law states that energy is conserved, the Second Law outlines the limitations of energy transfer and the natural tendency towards increased entropy.