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1a- Discuss the vaporization of water in standard condition at 298 K in term of: -...

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Chemistry

1a- Discuss the vaporization of water in standard condition at298 K in term of: - exothermicity and endothermicity - change ofentropy of the system and the surrounding - spontaneity of thereaction.

1b- Explain how the temperature and the composition of the twophases (liquid and vapour) influence the spontaneity of thevaporization of water.

Answer & Explanation Solved by verified expert
3.9 Ratings (419 Votes)
Water has a greater entropy than ice and so entropy favoursmeltingBut ice has a lower energy than water and so energy favoursfreezingIt is possible to predict what will happen by taking intoaccount the entropy of the surroundings in addition to the energyof the systemFreezing is an exothermic process energy is lost from thewater and dissipated to the surroundingsTherefore as the surroundings get hotter they are gainingmore energy and thus the entropy of the surroundings isincreasingThe amount by which the entropy of the surroundings hasincreased can be determined using the following principlethe entropy of the surroundings    See Answer
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