Cameron Miranda
The first law of thermodynamics, a formulation of the law of conservation of energy in the context of thermodynamic processes, can be applied to closed systems. This law is of great importance and generality and is thought of from several points of view. Textbook statements of the law often express it for closed systems, focusing on the distinction between transfers of energy as work and as heat. The first law of thermodynamics for closed systems can be applied to various real-world scenarios, such as the vapour compression refrigeration cycle or the Stirling cycle engine.
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What You'll Learn
The first law of thermodynamics is an energy conservation law
The first law of thermodynamics is a formulation of the law of conservation of energy in the context of thermodynamic processes. It is an energy conservation law, which means that energy cannot be created or destroyed, only transformed from one form to another. This law is of great importance and generality and is applicable to closed systems.
The first law of thermodynamics for closed systems can be understood as a conservation of energy principle. Energy is transferred between the system and its surroundings in the form of heat and work, resulting in a change in the internal energy of the system. This change in internal energy is the same as that for a reference adiabatic work process that links the initial and final states of the system. The reference process may be chosen arbitrarily from amongst all such processes.
The distinction between transfers of energy as work and as heat is central to the thermodynamics of closed systems. Heat and work are both energy transfer mechanisms that play an important role in the first law of thermodynamics. The law states that the change in the total energy stored in a system equals the net energy transferred to the system in the form of heat and work. This can be simplified as ΔU = U2-U1 = Q2 - W2, where Q represents heat transfer and W represents work.
The first law of thermodynamics can be applied to various practical scenarios, such as vapour compression refrigeration cycles, Stirling cycle engines, and heat engine processes. By considering the initial and final states of the system, along with the heat and work transferred, the first law can be used to solve problems and analyse energy transfers in closed systems.
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Energy transfers as work and heat
The first law of thermodynamics is a formulation of the law of conservation of energy in the context of thermodynamic processes. For a closed system, the distinction between energy transfers as work and as heat is central. The first law of thermodynamics states that the change in the total energy stored in a system equals the net energy transferred to the system in the form of heat and work.
The first law of thermodynamics for a closed system was expressed in two ways by Clausius. The first law postulates that a change in the internal energy of a system due to any arbitrary process, taking the system from a given initial thermodynamic state to a final equilibrium state, can be determined through the physical existence of a reference process that occurs purely through stages of adiabatic work.
Heat is also a form of energy transfer. The Sun generates energy, which is transferred through space to the Earth's atmosphere and surface as heat energy. There are three ways energy is transferred into and through the atmosphere: radiation, conduction, and convection. Radiation is the transfer of heat energy through space by electromagnetic radiation. Conduction is the transfer of heat energy from one substance to another or within a substance. Convection is the transfer of heat energy in a fluid.
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The role of internal energy
The first law of thermodynamics, also known as the law of conservation of energy, states that energy cannot be created or destroyed, only altered in form. This law applies to both open and closed systems.
Internal energy is a fundamental concept in the first law of thermodynamics. It refers to the total energy contained within a given system, encompassing the kinetic energy of molecules and the energy stored in chemical bonds. The internal energy of a system is influenced by heat and work done on or by the system. When heat is added to a system, its internal energy increases, and when the system performs work or releases heat, its internal energy decreases.
In a closed system, the first law of thermodynamics dictates that the change in internal energy is equivalent to the difference in internal energy between the final and initial states. This is true regardless of whether the process is adiabatic (without heat transfer) or non-adiabatic (with heat transfer). The first law for closed systems can be mathematically represented as:
$$\Delta U = U_2 - U_1 = Q - W$$
Where:
- $\Delta U$ is the change in internal energy,
- $U_2$ is the internal energy in the final state,
- $U_1$ is the internal energy in the initial state,
- $Q$ is the heat added to the system, and
- $W$ is the work done by the system.
The first law of thermodynamics provides a framework for understanding the behaviour of energy in closed systems and is a fundamental concept in the field of engineering thermodynamics.
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The mechanical approach
Born's mechanical approach recognises that when there is a transfer of matter between two systems, there is also a transfer of internal energy that cannot be separated into heat and work components. There can be pathways to other systems, distinct from the matter transfer, that allow heat and work transfer independent of and simultaneous with the matter transfer. In such cases, energy is conserved.
The first law of thermodynamics for a closed system can be expressed as:
> $\Delta U = U_2-U_1 = {}_{1}Q_{2} - {}_{1}W_{2}$
Where [latex]Q] is heat transfer in a process and [latex]W] is work. The change in the internal energy of a system is determined by the net energy transferred to the system in the form of heat and work.
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Application in heat engine processes
The first law of thermodynamics is a formulation of the law of conservation of energy in the context of thermodynamic processes. For a thermodynamic process affecting a thermodynamic system without transfer of matter, the law distinguishes two principal forms of energy transfer: heat and thermodynamic work. The law also defines the internal energy of a system, an extensive property for taking account of the balance of heat transfer, thermodynamic work, and matter transfer, into and out of the system.
The first law of thermodynamics is of great importance and generality and is consequently thought of from several points of view. Most careful textbook statements of the law express it for closed systems. The distinction between transfers of energy as work and as heat is central to the thermodynamics of closed systems.
The first law of thermodynamics can be applied to heat engine processes. A heat engine is a device that uses heat transfer to do work. Car engines and steam turbines that generate electricity are examples of heat engines. The first law of thermodynamics can be used to describe the processes of a simple heat engine. There are several simple processes, used by heat engines, that flow from the first law of thermodynamics. Among them are the isobaric, isochoric, isothermal, and adiabatic processes. These processes differ from one another based on how they affect pressure, volume, temperature, and heat transfer.
An isothermal process is a thermodynamic process in which no change in temperature takes place. A gas expanding isothermally, for example, does work on the surrounding, but its internal energy (as represented by the temperature) does not change, because enough heat flows in to balance out the energy expended in doing work. This is consistent with the first law of thermodynamics, because Q=W. An isothermal process occurs if a thermodynamic process in a gas occurs slowly enough so that the gas remains in thermal equilibrium with the surrounding at all times. The adiabatic process is, in some sense, the opposite of an isothermal process. In an adiabatic process, no heat transfer takes place (that is, Q=0). This may happen because the gas is well-insulated from the surrounding. It may also happen because the process occurs so quickly that no significant heat transfer can take place.
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