Thermochemistry

It's an exothermic reaction

It's an endothermic reaction

It's a sublimation reaction

It's a chemical change

Liquid to solid (freezing)

Solid to gas (sublimation)

Solid to liquid (melting)

Liquid to gas (vaporization)

Externally Pressure

Entropy

Volume

Temperature

The lower density of ice compared to liquid water ensures insulation of underlying water layers.

The higher heat capacity of ice compared--

Ice spontaneously melts without any addition of heat at standard conditions.

The temperature decreases as ice undergoes fusion into water.

Melting ice requires absorption of heat from the environment.

Ice releases heat as it melts into liquid water.

Water molecules dissociate into hydrogen and oxygen atoms.

The average velocity of water molecules significantly increases.

Kinetic energy within individual water molecules increases.

Intermolecular attractive forces between water molecules increase.

94 kJ

24 kJ

82 kJ

70 kJ

Entropy increases due to greater molecular disorder and freedom of movement upon melting.

Entropy decreases because molecules become more ordered as they form a liquid structure.

Entropy initially increases then decreases back as dynamic equilibrium is established between phases.

Entropy remains constant since temperature is unchanged during phase transition.

Sublimation

Deposition

Vaporization

Freezing

It decreases since higher pressure forces molecules apart easier, allowing them to vaporize at lower temperatures.

It first decreases then increases beyond its normal value due to fluctuations in intermolecular forces.

It increases because more energy is needed for water molecules to escape into vapor phase.

It remains unchanged as boiling point is solely dependent on water's chemical properties.