Assertion: The increase in internal encrgy (Δ E) for the vapourization of one mole of water at 1 atm and 373 K is zero. Reason: For all isothermal processes, Δ E = 0 .

Question

Assertion: The increase in internal encrgy (Δ E) for the vapourization of one mole of water at 1 atm and 373 K is zero. Reason: For all isothermal processes, Δ E = 0 . (A) If both assertion and reason are true and the reason is the correct explanation of the assertion (B) If both assertion and reason are true and the reason is not the correct explanation of the assertion (C) If assertion is true but reason is false (D) If both assertion and reason are false

Tardigrade Admin · Accepted Answer

At 373 K or 100° C, the water starts boiling and at this temperature the vaporization of water is an isothermal process. The internal energy change (Δ E), depend only on temperature, it follows that at constant temperature, the internal energy of the gas remains constant, i.e. Δ E is zero.

Q. Assertion : The increase in internal encrgy (ΔE) for the vapourization of one mole of water at 1 atm and 373K is zero. Reason : For all isothermal processes, ΔE=0.

If both assertion and reason are true and the reason is the correct explanation of the assertion

If both assertion and reason are true and the reason is not the correct explanation of the assertion

If assertion is true but reason is false

If both assertion and reason are false

At 373K or 100∘C, the water starts boiling and at this temperature the vaporization of water is an isothermal process. The internal energy change (ΔE), depend only on temperature, it follows that at constant temperature, the internal energy of the gas remains constant, i.e. ΔE is zero.

Q. Assertion : The increase in internal encrgy $(Δ E)$ for the vapourization of one mole of water at $1$ atm and $373 K$ is zero. Reason : For all isothermal processes, $Δ E = 0.$