Solution:The first law of thermodynamics, often called the law of conservation of energy, states that energy cannot be created or destroyed in an isolated system.
The total energy within a system can change forms (from kinetic to potential energy or vice versa), but the total amount of energy remains constant.
This concept underpins many physical processes and is fundamental in understanding energy transfer and transformation in closed systems.
For instance, when we burn fuel, it doesn't disappear but is transformed from chemical energy into heat and light energy.
Similarly, when we eat, our body converts the chemical energy in food into energy that our cells can use to function and grow.
This law contrasts with concepts like conservation of mass (from which it is distinct) and conservation of momentum, which are governed by different principles.