posted by Shelby on .
How much heat, in Kj, is required to melt 11.0g of ice, at -13.0 degrees C, and vaporize the H20, and rise the temperature of the steam to 114 degrees C. Need help. Anyone, please!
You need two formulas.
q needed within a phase is
[mass x specific heat in that phase x (Tfinal-Tinitial)].
For example to change T of 100 g liquid water at zero C to liquid water at 100 will require q = [100 x 4.184 x (100-0) = ?
q needed at a phase change is
[mass x heat fusion] at melting point or
[mass x heat vaporization] at boiling point.
Then add all of the q values for each phase change and each move in T within a phase together for the total.