we calculated the amount of enthalpy that needed to cool down an iron sample (100 g) from 1100oC to 0oC by throwing it into a bucket of ice water (ice + water). This enthalpy was -74.91 kJ. What is the minimal amount of ice (in grams) that has to be present to keep the bucket at 0C after it has equilibrated with the iron? You may assume that the bucket does not exchange heat with its surroundings (only with the iron).

Data: C(p, gamma)= 34 J/molK, C(p, alpha) = 38 J/molK, M(Fe) = 56 g/mol, M(ice) = 18 g/mol, = 6.048 kJ/mol