How much energy is required to melt 10.0 g of ice at 0.0°C, warm it to 100.0°C and completely vaporize the sample? The enthalpy of fusion of ice = 333 J g^-1 at 0 °C; the specific heat of water = 4.184 J g^-1 °C^-1; the heat of vaporization of water = 2260 J g^-1 at 100 °C.

Question

Quizplus · Accepted Answer

To melt the ice: 
Energy = mass*enthalpy of fusion 
Energy = 10.0 g * 333 J/g = 3330 J

To warm the water from 0°C to 100°C: 
Energy = mass*specific heat*ΔT 
Energy = 10.0 g * 4.184 J/g°C * (100°C-0°C) 
Energy = 4184 J

To vaporize the water: 
Energy = mass*enthalpy of vaporization 
Energy = 10.0 g * 2260 J/g = 22600 J

Total Energy = 3330 J + 4184 J + 22600 J = 30114 J

Therefore, the closest choice to the answer is A) 30100 J.

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