Statement I: : In isothermal process whole of the heat energy supplied to the body is converted into internal energy. Statement II: According to the first law of thermodynamics Δ Q = Δ U for an isothermal process.

Question

Statement I: : In isothermal process whole of the heat energy supplied to the body is converted into internal energy. Statement II: According to the first law of thermodynamics Δ Q = Δ U for an isothermal process. (A) Both statement I and II are correct. (B) Both statement I and II are incorrect. (C) Statement I is correct but statement II is incorrect. (D) Statement II is correct but statement I is incorrect.

Tardigrade Admin · Accepted Answer

In isothermal process, Δ T=0 and so Δ U=0. Thus Q=0+W=W.

Q. Statement I : : In isothermal process whole of the heat energy supplied to the body is converted into internal energy.
Statement II: According to the first law of thermodynamics $Δ Q = Δ U$ for an isothermal process.

Both statement I and II are correct.

Both statement I and II are incorrect.

Statement I is correct but statement II is incorrect.

Statement II is correct but statement I is incorrect.

In isothermal process, $Δ T = 0$ and so $Δ U = 0$ . Thus $Q = 0 + W = W$ .

Q. Statement I : : In isothermal process whole of the heat energy supplied to the body is converted into internal energy. Statement II: According to the first law of thermodynamics ΔQ=ΔU for an isothermal process.