Find the change in entropy of the h2o molecules when 1.38 kilograms of ice melts into water at 273 k. j/k (b) find the change in entropy of the h2o molecules when 1.38 kilograms of water changes into steam at 373 k. j/k (c) on the basis of the answers to parts (a) and (b), discuss which change creates more disorder in the collection of h2o molecules.

(a)

(b)

(c) Vaporization creates more disorder in the water molecules.

Explanation:

Given that:

mass of water,

transition temperature of ice into water,

transition temperature of water into steam,

We know:

Latent heat of fusion of ice,

Latent heat of vapourization of water,

Heat change during melting of ice:

Heat change during vaporization:

we have the equation of entropy change Δs:

where:

T= temperature in kelvin

dQ= change in heat energy

(a)

∴The change in entropy of the water molecules when 1.38 kilograms of ice melts into water at 273 K

.....................()

(b)

∴The change in entropy of the water molecules when 1.38 kilograms of water vaporizes at 373 K

.....................()

(c)

Vapourization of water creates more randomness and disorderliness in the molecules of the water because change in entropy is greater for vapourization and entropy change is the denotes randomness.

it is very well related to a lot of things but with my limited knowledge i can confidently say that the answer is space.