q=ms∆t
q= 33.136g x 4.184 J/gxC x 16.8C
q=2,329.17 J (liquid)
∆Hfus = 6.01 kJ/mole
use stoichiometry:
33.136 g | 1 mole H2O = 1.838 mole
| 18.02 H2O
1.838 mole | 6.01 kJ = 11.05 kJ
| 1 mole
q=33.136g x 2.108 J/gxC x 16.8C
q= 1,173.49 J (solid)
2,329.17 J + 11051.5 J + 1,173.49 J 14,554.1 J
2.32917 kJ + 11.05 kJ 1.17349 kJ = 14.55 kJ
1 kJ = 1,000 J
help? how do i calculate the heat of formation of a solid?
i only know how to find the heat of formation of a liquid.
here's what i have so far.
delta t= 16.8 degrees c
mass= 33.136 g
cp = 4.184 j/g degrees c
m cp delta t = -2329J (process is exothermic)
what do i do now?
1 answer
1 answer