2.10
Thermodynamic Processes
A thermodynamic process is a path through a sequence of states that takes a system from an initial state to a final state. In a cyclic process, the sy…
A thermodynamic system undergoes a change of state when one or more properties defining its state change.
Processes that go from the same initial state to the same final state via different paths are considered different processes.
In a cyclic process, the system returns to its initial state, so state functions like temperature, pressure, and volume return to their original values. However, the heat and work exchanged during the cycle can be nonzero.
In a reversible process, the system is constantly close to equilibrium, and any infinitesimal change can re-establish both the system and surroundings to their original states. Work in such a process is given by dwrev = -p dV, and heat dq, when divided by temperature, corresponds to the change in entropy.
An isothermal process keeps temperature constant throughout, while an adiabatic process involves no heat exchange, so q and dq are equal to zero.
An isochoric process holds volume constant, while an isobaric process holds pressure steady during the entire process. For a constant-pressure process, it's found that ΔH = qp.
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Q1: What happens to state properties during a cyclic thermodynamic process?
In a cyclic process, the system returns to its initial state, so state properties like temperature, pressure, and volume return to their original values. However, heat and work exchanged during the cycle can be nonzero. The net heat and net work over the complete cycle need not be zero, even though all state function changes equal zero.
Q2: How does a reversible process differ from an irreversible process?
A reversible process keeps the system infinitesimally close to equilibrium, allowing any infinitesimal change to restore both system and surroundings to original states. Work in reversible processes follows dwrev = -pdV. Irreversible processes proceed with finite changes and cannot restore the system and surroundings without external work, occurring when friction or finite compositional, pressure, or temperature changes are present.
Q3: What distinguishes an isothermal process from an adiabatic process?
An isothermal process maintains constant temperature by placing the system in a thermal bath at fixed temperature, while other properties like volume may change. An adiabatic process involves no heat exchange between system and surroundings, achieved using adiabatic walls, so q and dq equal zero. Both processes can change internal energy and work, but through different mechanisms.
Q4: Why is work zero in a constant-volume process?
In a constant-volume process, system volume remains fixed using rigid walls, so no pV work occurs. Since work is given by dwrev = -pdV, when dV equals zero, the work term becomes zero regardless of pressure changes. This contrasts with constant-pressure processes, where volume can change and work is performed on or by the system.
Q5: How is enthalpy related to heat in a constant-pressure process?
In a constant-pressure process, the heat absorbed or released equals the change in enthalpy: ΔH = qp. This relationship makes enthalpy particularly useful for analyzing chemical reactions and physical changes occurring at constant pressure, such as processes in open containers at atmospheric pressure.
Q6: What defines different thermodynamic process types?
Common process types are defined by what remains constant: isothermal processes hold temperature T constant, adiabatic processes maintain zero heat transfer (q = 0), isochoric processes keep volume V constant with zero work, and isobaric processes maintain constant pressure p. Each constraint determines how the system's energy and work are distributed during state changes.
Q7: How do different paths affect the relationship between initial and final states?
Processes connecting the same initial and final states via different paths are considered different processes. Although state functions like temperature, pressure, and volume depend only on initial and final states, the heat and work exchanged differ for each path. This distinction is central to understanding state functions and exact differentials in thermodynamics.