Question #440b7

1 Answer
Apr 10, 2017

Answer:

30.73 KJ.

Explanation:

use these equations:
#q = mcDeltaT# - for temperature change
#q = DeltaH_"fus/vap" * "moles"# - for phase changes

also, use these values:
#DeltaH_"fusion"# = 6.01 KJ/mol
(KJ needed per mole of water to change solid#harr#liquid)
#DeltaH_"vaporization"# = 40.7 KJ/mol
(KJ needed per mole of water to change liquid#harr#gas)
Specific heat of water = 4.18 J/g*C

First, you have to find the amount of heat energy required for each step.

Step 1: ice at -10 degrees to ice at 0 degrees
#q = mcDeltaT#
q = (10)(2.09)(10)
q = 209 J = .209 KJ

Step 2: ice at 0 degrees to water at 0 degrees
#q = DeltaH_"fus" * "moles"#
10 g water = .556 mol water (divide my molar mass which is 18g)
q = (6.01)(.556)
q = 3.34 KJ

Step 3: water at 0 degrees to water at 100 degrees
#q = mcDeltaT#
q = (10)(4.18)(100)
q = 4180 J = 4.180 KJ

Step 4: water at 100 degrees to steam at 100 degrees
#q = DeltaH_"vap"* "moles"#
q = (40.7)(.556)
q = 22.63 KJ

Step 5: steam at 100 degrees to steam at 120 degrees
#q = mcDeltaT#
q = (10)(1.84)(20)
q = 368 J = .368KJ

Now, add up all the values to get the final answer.
.209 + 3.34 + 4.180 + 22.63 + .368 = 30.73 KJ

This is a very helpful reference graph.

http://diagram.rogersvillegallery.com/phase-change-diagram-heating-curve-worksheet/