No heat enters or leaves he system at any time during the process, and the deformation is rapid enough that the process cannot be considered quasi-static. Once the final state is attained, there is no way of getting the system back to the initial state without also causing a change in the surroundings.iScience said:*edited*
Just realized that's not what i wanted to ask, sorry.
New Question: What is an irreversible adiabatic process? is it when the net q(sys) remains the same but there is heat transferred within the system?
Just to add to what Chet has said, you could think of an irreversible adiabatic expansion as a dynamic process in which one part of the system does work on another part, which takes the system out of equilibrium. Since it is adiabatic, the work done has to be at the expense of the system's internal energy. When the system returns to equilibrium the energy gained by the part on which work was done is distributed back to the system as a whole. This could be viewed heat transfer within the system.iScience said:*edited*
Just realized that's not what i wanted to ask, sorry.
New Question: What is an irreversible adiabatic process? is it when the net q(sys) remains the same but there is heat transferred within the system?
Sanky123 said:What is differece between free expansion and ordinary expansion ??
But how is this possible?Matterwave said:Free expansion means there's no external pressure or membrane inhibiting the expansion. In other words, a free expansion would be an expansion into a vacuum.
Sanky123 said:But how is this possible?
expansion in vaccume?
Thermodynamics is the branch of physics that deals with the relationships between heat, energy, and work. It studies how energy is transferred between different systems and how it affects the properties and behavior of matter.
The first law states that energy cannot be created or destroyed, only transferred or converted from one form to another. The second law states that the total entropy of a closed system will always increase over time. The third law states that as temperature approaches absolute zero, the entropy of a pure, perfect crystal becomes zero.
Heat refers to the transfer of thermal energy from one system to another, while temperature is a measure of the average kinetic energy of the particles in a system. In other words, heat is a form of energy, while temperature is a measure of how hot or cold something is.
There are four types of thermodynamic processes: isobaric (constant pressure), isochoric (constant volume), isothermal (constant temperature), and adiabatic (no heat transfer). These processes describe how a system changes as it exchanges heat and/or work with its surroundings.
Entropy is a measure of the randomness or disorder in a system. The second law of thermodynamics states that the total entropy of a closed system will always increase over time. Entropy plays a crucial role in determining the direction and efficiency of energy transfers and transformations in physical and chemical processes.