What is the change in entropy when 1gram of ice at 0° C is converted into water at the same temperature?
My attempt at the solution.
dS = dQ/T, where S is entropy, Q is heat energy and T is absolute temperature.
Again Q = mass X specific heat capacity X Change in temperature(ΔT)
T in the denominator is absolute temperature so 0+273 = 273K.
mass = 1 gm. I don't know what to substitute for sp.heat capacity? Whether sp.heat of water or sp.heat of ice? Again for ΔT, what values to substitute? Revered members can help.

 

Why does specific heat matter? Think about its definition. Then think about heat of fusion.

 

Thanks russ_hensel. So dS = 1X80(latent heat of fusion of ice)/273K which gives 0.293cal/K. Am i right?