I just need help with the last part of the problem. Thank you!   A sample containing 1200.0 grams of ice at -13.8°C is given 580.0 kJ of heat. ΔHfusion = 6.01 kJ/mol ΔHvap = 40.8 kJ/mol Specific heat of ice = 1.877 J/gK Specific heat of water = 4.184 J/gK Specific heat of steam = 2.013 J/gK. How much energy (in kJ) is needed to heat the 1200.0 grams of ice up to 0.00°C?  31.1 kJ How much energy (in kJ) is needed to melt 1200.0 grams of ice at 0.00°C to water at 0°C?  401 kJ How much energy (in kJ) is needed to heat the 1200.0 grams of water from 0.00°C to the boiling point of water?  502 kJ If you start at -13.8°C, what is the final temperature of the system after you have added the 580.0 kJ of heat? ? °C

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