Statement I: The enthalpy of formation of H₂O_(l) is greater than that of H₂O_(g).
Statement II: Enthalpy change is negative for the condensation reaction H₂O_(g) → H₂O_(l).

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Statement I and Statement II are true.

Statement I is false and Statement II is true.

Statement I is true and statement II is false.

Statement I and Statement II are false.

answer is A.

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Detailed Solution

(I) some amount of energy is used in the vapourization H₂O_(l)

(II) Molecules of gas are having high Kinetic energy, high disorder and weak attractive forces

on condensation , K.E decreases , randomness decreases , attractive forces becomes stronger energy is released

$\therefore\;\Delta H=-ve$

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