A piece of ice with mass 0.1 kg in temperature -10 celsius degree is put in a temperature of 17 celsius degree.
a) Find the heat that the ice absorbs until it melts.
b) Find the change of entropy from the beginning till it turns to water and reaches 17 celsius degree.The specific heat of ice is 2100 J/kgK and the specific heat of its melt is 33000 J/kg

For part (a) the heat absorbed per Kg is equal to the sum of: (1) the specific heat of ice times the delta in temp change to the melting point, plus (2) the specific heat of ice melt, plus (3) the specific heat of water times the temp change from freezing to the final temperature. Multiply this by the mass of water in Kg to get heat in Joules.

For part (b):

\Delta S = C_p \ln \frac {T_2} {T_1}


Where C_p is the heat capacity of the material, or your specific heat times mass of water.