First Law of Thermodynamics Question

AI Thread Summary
The first law of thermodynamics is expressed as ΔQ = ΔU + ΔW, where ΔQ represents the heat added to the system, ΔU indicates the change in internal energy, and ΔW signifies the work done by the system. This law emphasizes energy conservation, stating that the heat supplied is partially converted into internal energy and work. The confusion arises from the equation's format, but it fundamentally illustrates the relationship between heat, internal energy, and work. Understanding these terms is crucial for applying the first law in thermodynamic problems. Overall, the first law highlights the interplay between heat, energy, and work in thermodynamic systems.
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Homework Statement


The first law of thermodynamics states ΔQ = ΔU + ΔW. What does the ΔQ and the ΔW represent?


Homework Equations


ΔQ = ΔU + ΔW


The Attempt at a Solution


I've never seen the equation set up like this before so I'm a little confused. I said that ΔQ is the heat supplied to the system and ΔW is the work done by the system.
 
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First law of thermodynamics is basically an energy conservation law. It just states that heat that is added to the system is partially converted to system's internal energy and to perform work. That's all. ΔQ is heat added to the system, ΔU is change of internal energy (sum of all potential and kinetic energy of its particles) and ΔW is work done by the system.
 

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