Assertion: For an isothermal reversible process Q=-W i.e. work done by the system equals the heat absorbed by the system. Reason: Enthalpy change (Δ H) is zero for isothermal process.

Question

Assertion: For an isothermal reversible process Q=-W i.e. work done by the system equals the heat absorbed by the system. Reason: Enthalpy change (Δ H) is zero for isothermal process. (A) If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion. (B) If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion. (C) If the Assertion is correct but Reason is incorrect. (D) If the Assertion is incorrect and Reason is correct.

Tardigrade Admin · Accepted Answer

In an isothermal process change in internal energy

(Δ E)

is zero (as it is a function of temperature).

∴

According to first law of thermodynamics

∵ Q + W = Δ E

. Hence

Q = - W (

if

Δ E = 0)

If a system undergoes a change in which internal energy of the system remains constant (i.e.

Δ E = 0

) then

- W = Q

. This means that work done by the system equals the heat

Q. Assertion: For an isothermal reversible process Q=−W i.e. work done by the system equals the heat absorbed by the system. Reason : Enthalpy change (ΔH) is zero for isothermal process.

If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.

If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.

If the Assertion is correct but Reason is incorrect.

If the Assertion is incorrect and Reason is correct.

Q. Assertion: For an isothermal reversible process $Q = - W$ i.e. work done by the system equals the heat absorbed by the system.
Reason : Enthalpy change $(Δ H)$ is zero for isothermal process.