(c) By what means can the internal energy of a closed system increase?

Verified step by step guidance

1. Understand that internal energy (U) of a closed system can change through heat (q) and work (w) based on the first law of thermodynamics.
2. Recall the first law of thermodynamics: \( \Delta U = q + w \), where \( \Delta U \) is the change in internal energy.
3. Identify that internal energy increases when the system absorbs heat (q > 0) from the surroundings.
4. Recognize that internal energy also increases when work is done on the system (w > 0), such as compression work.
5. Conclude that both heat absorption and work done on the system contribute to an increase in internal energy.

Key Concepts

Internal Energy

Internal energy is the total energy contained within a system, encompassing both kinetic and potential energy of the particles. It is a state function, meaning it depends only on the current state of the system, not on how it reached that state. Changes in internal energy can be observed through heat transfer and work done on or by the system.

First Law of Thermodynamics

The First Law of Thermodynamics states that energy cannot be created or destroyed, only transformed from one form to another. In a closed system, the change in internal energy is equal to the heat added to the system minus the work done by the system. This principle is fundamental in understanding how energy transfers affect a system's internal energy.

Heat and Work

Heat and work are two primary means by which energy can be transferred into or out of a system. Heat refers to energy transfer due to temperature differences, while work involves energy transfer resulting from forces acting over distances. Both processes can lead to an increase in a system's internal energy, depending on the direction of energy flow.