thermodynamics and thermochemistry- adiabatic irreversible process and isochoric irreversible process
we know that heat and work done are path function properties and internal energy is state function property.
in adiabatic irreversible process it was said that since heat change is 0, therefore through first law of thermodynamics work done will be equal to internal energy but since internal energy is state function property, work done will also become state function property which is wrong and hence same state change cannot be caused by adiabatic reversible as well as adiabatic irreversible process. but in isochoric process where work done was zero and heat change was being equal to internal energy, it was said that isochoric reversible process is equal to isochoric irreversible process and delta Q reversible = delta Q irreversible; which makes heat change also state change property and not path change property. how is it true that heat change can be both state change as well as path change but work done cannot?
In irreversible isochoric: q = ∆E
In irreversible adiabatic: W = ∆E
Both equality can be valid in two cases:
Case 1: Both reversible and irreversible are same path leads to same change of state which is the case of irreversible isochoric process.
Case 2: Both reversible and irreversible are different path leads to different change of state which is the case of irreversible adiabatic process.