Statement 1: The increase in internal energy (Δ E) for the vaporisation of 1 mole of water at 1 atm and 373K is zero. Statement 2: For all isothermal processes Δ E = 0.

Question

Statement 1: The increase in internal energy (Δ E) for the vaporisation of 1 mole of water at 1 atm and 373K is zero. Statement 2: For all isothermal processes Δ E = 0. (A) If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation of the statement 1 (B) If both Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1 (C) If Statement 1 is true but Statement 2 is false (D) If Statement 1 is false but Statement 2 is true

Tardigrade Admin · Accepted Answer

The statement 1 that the increase in internal energy for the vaporisation of lmole of water at 1 atm and 373 K is zero is true because for all isothermal process internal energy is zero.

Q. Statement 1: The increase in internal energy $(Δ E)$ for the vaporisation of 1 mole of water at 1 atm and $373 K$ is zero.
Statement 2: For all isothermal processes $Δ E = 0.$

If both Statement 1 and Statement 2 are true and the statement 2 is the correct explanation of the statement 1

If both Statement 1 and Statement 2 are true but statement 2 is not the correct explanation of the statement 1

If Statement 1 is true but Statement 2 is false

If Statement 1 is false but Statement 2 is true

The statement 1 that the increase in internal energy for the vaporisation of lmole of water at 1 atm and $373 K$ is zero is true because for all isothermal process internal energy is zero.

Q. Statement 1: The increase in internal energy (ΔE) for the vaporisation of 1 mole of water at 1 atm and 373K is zero. Statement 2: For all isothermal processes ΔE=0.