A 4.00-kg silver ingot is taken from a furnace, where its temperature is 750.0o C, and placed on a large block of ice at 0.0o C. Assuming that all the heat given up by the silver is used to melt the ice, how much ice is melted?

Solution 59E Introduction In this problem we will use the concept of calorimetry, that is, since no heat is lost, the amount of energy released by silver will be equal to the amount of heat taken by ice to melt. Step 1 The heat released by silver is given by Q s m c s s s Here we have m = 4.00 kg s c s 234 J/kg.K And T = S750.0 0) = 750.0°C = 750.0 K So Q = (4.00 kg)(234 J/kg.K)(750.0 K) = 7.02 × 10 J 5 s Step 2 Now suppose the mass of ice that will melt is m, and the latent heat of ice fusion is L = 334 × 10 J/kg Hence we have 3 Q i m(334 × 10 J/kg)