State the first law of thermodynamics in your own words. What equation defines the change in the

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State the first law of thermodynamics in your own words....

Key Concepts

First Law of Thermodynamics

The first law of thermodynamics is a statement of energy conservation. It asserts that the change in a system's internal energy is equal to the heat added to the system minus the work done by the system on its surroundings. This law implies that energy can neither be created nor destroyed, only transformed from one form to another.

Internal Energy

Internal energy is the total energy contained within a system and encompasses all forms of energy including kinetic and potential energies of the molecules. It represents the sum of all the microscopic forms of energy present in a system, which in turn determines the system's state.

Heat

Heat is the form of energy transferred between systems (or a system and its surroundings) due to a temperature difference. In the framework of the first law, heat added to the system is denoted by Q and is considered positive when energy enters the system.

Work

Work is the energy transferred when an external force acts over a distance, often resulting in energy leaving the system. In the first law of thermodynamics, work is usually represented by W. It is generally taken as positive when the system does work on the surroundings, thereby reducing the system’s internal energy.

Sign Conventions

The sign conventions in the first law are crucial for correctly accounting for energy exchanges. Heat (Q) is positive when added to the system, while work (W) is positive when performed by the system, which means the system loses energy. Thus, the change in internal energy is given as ?U = Q - W.

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