[krazyxazn]

How much energy does it take to convert 1.000 kg of steam at 300.0 ^oC ice at – 32.0 ^oC?

[Specific heat capacities: ice, 2.1 J/g· ^oC; liquid, 4.2 J/g· ^oC; steam, 2.0 J/g· ^oC; ? Hvap = 40.66 kJ/mol; ? Hfus = 6.01 kJ/mol]

Formulas:
q = mass x  specific heat  x change in temp
q = moles x Heat of phase change

This is my work, I don't know if it's right or not:

1kg x 10³ = 1000g
? mol H2O = 1000g / 18.01528 = 55.40166 mol H2O

q= 1000g (2 J/g) 200 C = 400,000 J / 1000 = 400 kJ
q= 55.40166 mol H₂0 ( -40.66 kJ ) = -2252.631579 kJ
q= 1000g (4.2 J/g) 100 C = 420,000 J / 1000 = 420 kJ
q= 55.40166 mol H₂0 ( -6.01 kJ) = -332.9639766 kJ
q= 1000g (2.1 J/g) 32 = 67200 / 1000 = 67.2 kJ
_______________________________________
-1698 kJ total energy

EDIT:
I found out what was wrong. I didn't calculate my temperatures correctly. I did initial - final instead of final - initial. My Final Answer: -3,471,200 J

[Yggdrasil]

Instead of relying on the actual numbers to figure out the sign of q, use your chemistry intuition.  In each of these processes, think about whether the molecules are gaining energy (q is positive) or losing energy (q is negative).