Calculate the entropy change in the melting of 1 kg of ice at `0^(@)C` in SI units. Heat of funsion of ice = 80 cal `g^(-1)`.

The entropy change in melting 1g of ice at 0^@C . (Latent heat of ice is 80 cal g^(-1) )

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.

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.

Calculate the entropy change when 20.0 g of ice changes to liquid water at 0°C. The heat of fusion is 80.0 cal g^(-1) .

Calculate the amount of heat required to convert 10g of ice at - 10^@C to water at 5^@C (latent heat of fusion of ice = 80 cal g^(-1) , specific heat of ice = 0.5).

Calculate change in entropy when 5g of pure ice melts to form water at 0^(@)C Given latent heat of ice is 80cal//g at 0^(@)C .

An iron ball of mass 0.2 kg is heated to 10^(@)C and put into a block of ice at 0^(@)C . 25 g of ice melts. If the latent heat of fusion of ice is 80 cal g^(-1) , then the specific heat of iron in cal g^(-1^(@))C is