Question

Need help with this practice problem. I got the values for the gas to liquid and liquid to solid. Don't know how to do the rest? Heat of Vap and fusion too? No idea!
What is the enthalpy change during the process in which 100.0 g of
water at 50.0 C is cooled to ice at 30.0 C?

The specific heats of ice, liquid water, and steam are 2.03 J/g-K, 4.18 J/g-K, and 1.84 J/g-K,
respectively. For H2O, Hfus = 6.01 kJ/mol and Hvap = 40.67 kJ/mol.

Please show the work. I know the answer is 60.4kJ
Thank you!

Answer 1

You have the phase changes. What you need is heat lost/gained within a phase. For both liquid and solid phase use this.
q = mass liquid H2O x specific heat H2O x (Tfinal-Tinitial)

q = mass ice x specific heat ice x (Tfinal-Tinitial)

By the way, ice at 30 C doesn't make sense. Neither does vap at 50 (it's a liquid there and not a gas).