Question #440b7
1 Answer
30.73 KJ.
Explanation:
use these equations:
also, use these values:
(KJ needed per mole of water to change solid
(KJ needed per mole of water to change liquid
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 = (10)(2.09)(10)
q = 209 J = .209 KJ
Step 2: ice at 0 degrees to water at 0 degrees
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 = (10)(4.18)(100)
q = 4180 J = 4.180 KJ
Step 4: water at 100 degrees to steam at 100 degrees
q = (40.7)(.556)
q = 22.63 KJ
Step 5: steam at 100 degrees to steam at 120 degrees
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.