Q.For isothermal process,

No, heat exchange is not possible in an adiabatic process — that is exactly its defining condition (q = 0).

An adiabatic process is defined as one that occurs without any transfer of heat between the system and its surroundings — the system is thermally insulated. This is achieved either by carrying out the process very rapidly (no time for heat exchange) or by physically insulating the system. Under the first law of thermodynamics, ΔU = q + w; for an adiabatic process q = 0, so ΔU = w — any change in internal energy (and …

The word 'isothermal' is built from 'iso-' (same) + 'thermal' (temperature) — the defining condition is that temperature stays constant throughout the process.

Thermodynamic processes are classified by which quantity is held constant:

• Isothermal process: temperature is constant, Delta T = 0 (but heat q and work w individually need not be zero — for an ideal gas, since internal energy depends only on T, Delta U = 0 too, so q = -w by the first law)
• Adiabatic process: no heat exchange with surroundings, q = 0
• Isochoric process: constant volume
• Isobaric process: constant pressure …

Isothermal ⇒ temperature constant ⇒ dT = 0.

"Iso-thermal" literally means "same temperature": the process is carried out in such a way that the temperature of the system remains constant throughout, i.e. $dT = 0$ (and hence $dU = 0$ for an ideal gas, since internal energy depends only on T). This is distinct from an isobaric pro …

'Isothermal' literally means 'same temperature', so the defining condition is that temperature does not change during the process, i.e. delta T = 0.

In thermodynamics, processes are classified by what is held constant:

• Isothermal: temperature (T) is constant throughout, so delta T = 0. This does NOT require q = 0 (heat can still flow to keep T constant, e.g. during isothermal expansion of an ideal gas).
• Adiabatic: no heat exchange with surroundings, q = 0 (this is what option (a)/(b) describe, a different process type). …

In an adiabatic process, the system is thermally isolated so that q = 0 -- any change in internal energy comes entirely from work done on or by the system.

For an adiabatic process, the condition is that no heat (q) enters or leaves the system: $q = 0$. From the first law of thermodynamics, $\Delta U = q + w$, this reduces to $\Delta U = w$ for an adiabatic process -- the entire change in internal energy equals the work done on/by the syste …

For a reversible adiabatic process, ΔS = 0.

An adiabatic process is one in which no heat enters or leaves the system, i.e. q = 0.

For a reversible process, the change in entropy is defined as:

ΔS = q_rev / T

Since q_rev = 0 for an adiabatic process, substituting into the formula gives ΔS = 0/T = 0.

…

'Adiabatic' means thermally insulated — no heat transfer occurs, so q = 0.

In thermodynamics, a process can be classified by what is held constant or exchanged:

• Isothermal: ΔT = 0 (temperature constant).
• Isobaric: ΔP = 0 (pressure constant). …

In an adiabatic process, q = 0 -- the system is thermally insulated, so all change in internal energy comes from work.

In thermodynamics, a system can exchange energy with its surroundings as heat (q) and/or as work (w). An adiabatic process is one carried out in a system that is thermally insulated from its surroundings, so that no heat can flow in or out during the process (q = 0).

From the first law of thermodynamics, ΔU = q + w. For an adiabatic process, since q = 0:

ΔU = w

…

'Adiabatic' means no heat transfer occurs between system and surroundings, so the defining condition is $q = 0$.

In thermodynamics, a process is called adiabatic when the system is thermally insulated from its surroundings, so that no exchange of heat takes place between them during the process; the defining condition is $q = 0$. (Temperature, pressure and work can still change during an adiabatic process — e.g. adiabatic compression raises temperature, so $\Delta T \neq 0$ in general, ruling out (a); pressure and work also generally change, r …

Adiabatic literally means 'no heat passes through' — the defining condition is q = 0, not ΔT, ΔP, or W being zero.

In thermodynamics, a process is classified by what is held constant or excluded:

• Isothermal: ΔT = 0 (temperature constant).
• Isobaric: ΔP = 0 (pressure constant).
• Adiabatic: q = 0 (no heat exchanged with the surroundings) — the system is thermally insulated.
• Isochoric: ΔV = 0 (volume constant). …