3 Laws of Thermodynamics
1. The First Law of Thermodynamics
The First Law of Thermodynamics, also known as the Law of Energy Conservation, states that energy cannot be created or destroyed, only transformed from one form to another. This means that the total energy of an isolated system remains constant.
Example: When you burn a piece of wood, the chemical energy stored in the wood is converted into heat, light, and other forms of energy. The total amount of energy before and after the burning remains the same.
2. The Second Law of Thermodynamics
The Second Law of Thermodynamics states that in any energy transfer or transformation, the total entropy of a closed system will always increase over time. Entropy is a measure of disorder or randomness. This law implies that natural processes tend to move towards a state of greater disorder.
Example: When you mix hot water and cold water, the hot water cools down and the cold water warms up until both reach the same temperature. The process is irreversible, and the system becomes more disordered as the temperature differences disappear.
3. The Third Law of Thermodynamics
The Third Law of Thermodynamics states that as the temperature of a system approaches absolute zero (0 Kelvin), the entropy of the system approaches a minimum value. This law implies that it is impossible to reach absolute zero in a finite number of steps.
Example: In a perfectly ordered crystal at absolute zero, all motion would cease, and the entropy would be at its lowest possible value. However, achieving this state is practically impossible due to the limitations of cooling processes.