(a) According to the first law of thermodynamics, what quantity is conserved?

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The first law of thermodynamics is a version of the law of conservation of energy, adapted for thermodynamic systems.

It states that energy cannot be created or destroyed in an isolated system.

The first law is often expressed as \( \Delta U = Q - W \), where \( \Delta U \) is the change in internal energy of the system, \( Q \) is the heat added to the system, and \( W \) is the work done by the system.

According to this law, the total energy of an isolated system is constant.

Therefore, the quantity that is conserved according to the first law of thermodynamics is energy.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 in an isolated system. Instead, energy can only be transformed from one form to another. This principle is fundamental in understanding how energy flows in physical and chemical processes.

Internal Energy

Internal energy is the total energy contained within a system, including kinetic and potential energy at the molecular level. According to the First Law of Thermodynamics, any change in the internal energy of a system is equal to the heat added to the system minus the work done by the system on its surroundings. This concept is crucial for analyzing thermodynamic processes.

Work and Heat

In thermodynamics, work and heat are two ways energy can be transferred between a system and its surroundings. Work refers to energy transfer that occurs when a force is applied over a distance, while heat is the energy transferred due to a temperature difference. Understanding these concepts is essential for applying the First Law of Thermodynamics to real-world scenarios.

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