Question

How much heat is evolved in converting 1.00 mol of steam at 155.0 ∘C to ice at -45.0 ∘C? The heat capacity of steam is 2.01 J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).

Answer 1

Let's see if you can do this yourself.
heat at phase change is
q = mass x heat vaporization at boiling point or
q = mass x heat fusion at freezing point.

Between phases it is
q = mass x specific heat x (Tfinal-Tinitial).
Now you have steam at 155 so it must go "within the phase" to 100 so that is equation 3.
Then you change from steam vapor to steam liquid. That's a phase change at the boiling point. Use equation 1.
Then you change T from 100 to zero C. That's equation 3 again.
At zero it freezes so that's a phase change from liquid to solid and you use equation 2.
Then you go from zero with a solid to -45 with a solid. That's equation again.
Then add all of the q values together.

Answer 2

I'm still not getting the correct answer.

Answer 3

I'm getting 5.65 kJ

Answer 4

Post your work for each step and I'll check it.

Answer 5

Check your arithmetic. I It looks like you have the right digits (close anyway) but off by a factor of 10. You don't show what you're using for delta H vap or delta H fusion. I used 18 g for a mole of H2O, 334J for delta H fusion and 2257J for heat vap and 4.18 for specific heat liquid water.