How do you calculate the change in entropy for non-constant temperature?

Question

For example, calculate the change in entropy in metling 1 kg of ice from 173K to 273K. (Specific heat: 2.05)

Answer 1

Here the ice is heated from 173 k (-100 C) to ice of 273 K (0 C) and changed into water at 273 K. The entropy will increase as disorder increased. heat supplied forms to parts, one that varies from 173 to 273 K and at constant temp - latent heat.
dQ = m L + m cp dT

change in entropy

ds= dQ / T = [m L/ T] + integral [m cp dT] / T (173 to 273 K)

L = latent heat of ice 334 KJ/Kg
Cp= specific heat of ice =2.05 KJ/kg. K

ds= [m L/ T] + [m cp] log [ T ] (173 to 273 K)
ds= [m L/ T] + [m cp] log [ 273 - 173 ]
ds= [1*334 / 273] + [1*2.05 ] log [ 100 ] K Joule/deg K
ds= 1.223 + 9.44 = 10.663 KJoule/deg K
answer

Answer 2

entropy in simple terms potential chaos. whilst they say something like entropy continuously will boost it potential that the device gets extra chaotic. in simple terms think of of a bomb as an occasion it starts off with low entropy yet on the top entropy is rather severe. Ice is rather uniform in comparison to water, this is molecules are set in neat rows yet because it melts they start flowing over one yet another turning out to be much less uniform therefor entropy has greater. same element is going for the splattering of an egg. Its very uniform before everything yet on the top the egg is in each and every single place.

Answer 3

That's easy, read the book...