Question

Consider the specific heats
CH2O(s) = 2.09 J/g ¡¤◦ C. CH2O(§¤) =4.18 J/g ¡¤◦ C. CH2O(g) = 2.03 J/g ¡¤◦ C.
The heat of fusion for water is 334 J/g and the heat of vaporization for water is 2260 J/g. Calculate the amount of heat absorbed when 86 g of steam at 133◦C are completely converted to ice at −27◦C.
Answer in units of kJ

Answer 1

An easy but long problem.
You have two formulas to use for this.
Within a phase (all gas, all liquid, all solid),
q = mass x specific heat x (Tfinal-Tinitial)

At a transition point:
At the boiling point is is
q = mass x heat vaporization

At the melting point it is
q = mass x heat fusion.

Then add the qs for the total.