Answer:
The first law of thermodynamics, also known as the law of conservation of energy, states that energy cannot be created or destroyed, only transferred or transformed from one form to another. In other words, the total energy of a closed system and its surroundings remains constant.
When applying this law to a system/surrounding model, the energy exchanged between the system and its surroundings can take different forms, such as heat, work, or a combination of both. For example, if a gas is compressed in a piston, work is done on the gas by the surroundings, increasing the internal energy of the gas. Alternatively, if a gas is heated, energy is transferred to the gas from the surroundings, increasing the internal energy of the gas.
Overall, the first law of thermodynamics serves as a fundamental principle in the study of thermodynamics, allowing us to analyze and predict energy transfers and transformations in various physical and chemical systems.
Step-by-step explanation: