Explain, why-one feels ice cream at `0^(@)C` colder than water at `0^(@)C` ?

Explain the following: Why do soft drink bottles cool better in ice at 0^(@)C than water at 0^(@)C ?

Calculate the entropy change (DeltaS) when 1 mol of ice at 0^(@)C is converted into water at 0^(@)C . Heat of fusion of ice at 0^(@)C is 1436 cal per mol.

What is the resulting temperature when 150 g of ice at 0^(@)C mixed with 300 g of water at 50^(@)C ?

Heat energy is supplied at a constant rate to 100 g of ice at 0^(@)C . The ice is converted into water at 0^(@)C in 2 minutes. How much time will be required to raise the temperature of water from 0^(@)C" to "20^(@)C ? [Given : sp. Heat capacity of water 4.2g^(-1)""^(@)C^(-1) , sp. latent heat of ice = 336Jg^(-1) ]

Statement- 1 : Potential energy of water at 0^(@)C is more than ice at 0^(@)C . Statement- 2 : Heat given to melt ice at 0^(@)C is used up in increasing the potential energy of water molecules formed at 0^(@)C .

Explain why : Ice at zero degree centigrade has greater cooling effect than water at 0^@C .

Soft drinks are cooled by placing them in ice rather than water at 0^@C . Why?

Why does a bottle of soft drink cool faster when surrounded by ice cubes than by ice cold water, both at 0^(@)C ?

50 gram of ice at 0^(@) C is mixed with 50 gram of water at 60^(@)C , final temperature of mixture will be :-

In an insulated vessel, 250g of ice at 0^(@)C is added to 600g of water at 18.0^(@)C .a. What is the final temperature of the system? B. How much ice remains when the system reaches equilibrium?