Question

What is meant by a state function? Give an example.

Short answer

A state function is a property of a system that depends only on its current state and is determined entirely by the values of the variables that define the state. The change in a state function during a process depends only on its initial state and final state, not on the path taken. Examples of state functions include internal energy (U) and entropy (S), as their changes (\( \Delta U \) and \( \Delta S \)) during a process depend only on the initial and final states, not the path taken.

Step-by-step solution

Definition of a State Function

A state function is a property of a system that depends only on its current state, which means it is determined entirely by the values of the variables that define the state, and not by the path the system took to reach the state. The change in a state function during a process depends only on its initial state and its final state, not on the intermediate states or the path taken during the process.

Example of a State Function

A common example of a state function is the internal energy (U) of a system. The internal energy of a system depends only on its current state, such as its temperature, pressure, and volume. So if a system undergoes a process, the change in internal energy (\( \Delta U \)) will depend only on the initial and final states of the system, not the path taken to get there. Another example of a state function is the entropy (S) of a system. Like the internal energy, the entropy of a system depends only on its current state, and the change in entropy (\( \Delta S \)) during a process depends only on the initial and final states, not the path taken.

Key concepts

Internal Energy

Internal energy is a key concept in the study of thermodynamics, which refers to the total energy contained within a system. It encompasses all forms of energy, such as kinetic energy, which is associated with the motion of particles within the system, and potential energy, which is related to the position of these particles or their arrangement. One important aspect of internal energy is that it is a state function.

This means that the internal energy of a system is determined by the state of the system itself, characterized by variables such as temperature, pressure, and volume. The symbol used to represent internal energy is usually 'U'. When a system undergoes any kind of change, the change in internal energy, denoted as \( \triangle U \), is independent of the process by which the system changed. It depends solely on the initial and final states of the system.

For example, whether a quantity of gas is heated rapidly or slowly, if both processes start and end at the same state, the change in internal energy will be the same. This is crucial for calculating energy changes in physical and chemical processes because it simplifies the computations to only require knowledge of the endpoint conditions.

Entropy

Entropy is a somewhat more abstract concept in thermodynamics, often associated with the degree of disorder or randomness in a system. It is a measure of how dispersed the system's energy is among its particles. Like internal energy, entropy is also a state function and is represented by the symbol 'S'.

The change in entropy of a system, expressed as \( \triangle S \), is not dependent on how a system reaches its final state but rather the comparison between the initial and final states themselves. The second law of thermodynamics states that for any natural thermodynamic process, the total entropy of the universe must increase, implying that processes tend to move towards greater disorder.

In practical terms, this means that if you have a closed system where energy is transformed, such as when ice melts into water, the change in entropy can be calculated by considering just the states of solid ice and liquid water, instead of the entire melting process. The concept of entropy is pivotal in understanding not only energy transfer but also the fundamental direction of natural processes.

Thermodynamics

Thermodynamics is a branch of physics that deals with the relationships between heat, work, temperature, and energy. The laws of thermodynamics govern the principles that oversee these relationships and dictate the direction of heat transfer, the efficiency of engines, and the feasibility of chemical reactions.

At its core, thermodynamics is built on the concept of state functions like internal energy and entropy. These functions are fundamental to understand how energy is conserved and how processes proceed towards equilibrium. For example, the first law of thermodynamics, also known as the law of energy conservation, states that energy cannot be created or destroyed in an isolated system, which directly relates to internal energy as a state function.

Moreover, the concept of state functions allows us to use equations to describe the state of a system and predict changes without worrying about the specific mechanisms or paths taken. This approach makes it possible to analyze complex systems and processes in a much more manageable way, laying the groundwork for advancements in fields ranging from engineering to biochemistry.