The molar heat of fusion for water is 6.008 kJ/mol. How much
energy would be required to melt 94.0 g of ice?
2007-06-13 18:10:19 · 4 answers · asked by sexxxxxxy4u 2 in Science & Mathematics ➔ Chemistry
so the r.m.m of water = 18
so the 94 = 94/18=5.2222 moles
6.008=energy/5.22222
6.005*5.2222=energy
31.359 kilojoules
2007-06-13 18:17:50 · answer #1 · answered by casim 2 · 0⤊ 0⤋
94.0 g ice = X mols of ice. (water is 18.14 g/mol)
therefore X mols times 6.008 kJ /mol = kJ required.
2007-06-13 18:15:38 · answer #2 · answered by Alan V 3 · 0⤊ 0⤋
Determine moles of water then multiply by molar heat of fusion
94g/[18g/mol] x 6.008 kJ/mol = 31.375 kJ
2007-06-13 18:18:28 · answer #3 · answered by Flying Dragon 7 · 0⤊ 0⤋
I am doing well, thank you for asking.
2015-05-14 09:15:37 · answer #4 · answered by Nick Romanowski 1 · 0⤊ 0⤋