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The energy of a system has always been a mystery, how it comes, where it goes, and all the questions like this. That is why there is some research and laws regarding this energy conversion. This energy conversion and the system, how it works, come under the segment of a particular physics. This physics is thermodynamics, which deals with the response of a large-scale system. These responses need to be observed and must be measured during the experiment. In The first law of thermodynamics, energy and heat are discussed.
Thermodynamics
It is very important to know about thermodynamics before knowing its different laws and equations. Thermodynamics is that part of physics where people deal with heat, temperature, work, and their relationship with energy, physical properties, and entropy of the particular matter.
Here, the states of a matter get described when external heat is provided to it, and the temperature increases, then the matter performs some work, and that is why there is a difference between provided heat and the result you get. This heat and work relationship is known as thermodynamics.
The first law of thermodynamics
The first law of thermodynamics states that energy cannot be created nor destroyed; this can only be transferred from one matter to another and from one state to another. Also, the changes in internal energy in the equilibrium state of the matter are equal to the difference between heat provided to the matter and the work done by the matter.
For an isolated system, the equilibrium state of the changes in internal energy depends on the heat provided to the system and the work done by the system. By differentiating the heat provided to the system and the work done by the system, you will get the equilibrium of the changes in the internal energy of the isolated system.
Internal Energy
The changes in energy of a matter or a system during providing heat and performing the work are known as internal energy. As per the first law of thermodynamics, these changes in internal energy remain in an equilibrium state based on the heat provided to the isolated system and the work performed by the system.
This energy is in thermodynamics, which cannot be created or destroyed. In any particular system, one state of energy can get converted to another and keep the system’s equilibrium.
Equation of The First Law of Thermodynamics
The most asked question about this topic is what is the exact equation of the first law of thermodynamics? To answer and describe this, we need to explain the relationship between internal energy, heat, and the work done by the system.
The first law stated that the changes in internal energy are equal to the difference between the heat provided to the system and the work performed by the system to keep the system’s equilibrium. So, the equation will also contain these three terms.
The equation will be as the changes in internal energy = The heat provided to the system – Work performed by the system.
This can also be written as
E2 is the changed energy after providing heat to the system, and E1 is the energy before the heat is provided and work performed.
∆U is denoted as the changes in the internal energy, Q is the heat provided to the system, and W is the work performed by the system to keep the equilibrium of the heat and energy of the system.
Usage Of the First Law of Thermodynamics
Any physical property of a matter or a system has some usage in daily lives; this law and property is also not an exception. That is why this is also required to discuss the daily usage of the first law of thermodynamics.
Electric bulbs are one of the best examples of daily life usage of this property. In this case, electric energy gets converted into light energy inside a bulb.
A heat engine is also one more example, as, in a heat engine, the thermal energy gets converted into mechanical energy; this one also follows the first law of thermodynamics.
Also, for a plant, this physical property of a system works during photosynthesis. During this event, the sun’s radiant energy gets converted into chemical energy.
Limitations
Like all other physical properties of a matter and a system, this law also has some limitations. This law cannot explain the change of state of a matter or the system providing the heat. Also, the heat flow from the hot end to the cold end is not explainable with the help of the first law of thermodynamics.
Conclusion
The first law of thermodynamics describes the internal energy change of an isolated system. This energy change happens due to the heat or any other energy provided to the system. And after receiving the heat, the system performs some work; the difference between the heat provided to the system and the work done by the system is the changes in internal energy. The equation E2 – E1 = ∆U=Q-W describes every individual to keep the system’s equilibrium.
