You have to heat all of the ice to 0, then melt it.
Heat=mcDeltatemp+ Hf*m
= m(2.01*(21)J/g + 6010J/mol*1mol/18g)
solve for m in grams
How many grams of ice at -20.1C can be completely converted to liquid at 9.9C if the available heat for this process is 4.58×103 kJ?
For ice, use a specific heat of 2.01 J/(g*C) and Heat of Fusion is = 6.01 kJ/mol.
1 answer
1 answer