In an isothermal change, the temperature of the system remains unchanged. Heat can be exchanged with the surroundings to ensure the temperature remains constant while the system undergoes expansion or compression.
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In an adiabatic change, no heat is exchanged with the surroundings, so heat remains unchanged. However, the temperature of the system can change due to work done on or by the system.
The concept of internal energy is derived from the first law of thermodynamics. This law, also known as the law of energy conservation, defines internal energy as the total energy contained within a system.
A fast-moving object has more kinetic energy compared to a slow-moving object of the same mass because kinetic energy is directly proportional to the square of the object’s velocity. This means that even a small increase in velocity results in ...
Work is the transfer of energy from one object to another or the conversion of energy from one form to another. In the examples, the cricket ball does work on the wicket by transferring its kinetic energy to it. Similarly, ...