If 13.4 kJ of energy are added to 1.00 kg of ice at 0 degrees Celsius, how much water at 0 degrees Celsius is produced? How much ice is left? The molar heat of melting is 6.01 kJ/mol.
So... 6.01 kJ -> 1 mol (6.01 kJ of energy can melt 1 mole of ice)
Then... 13.4 kJ -> x (How many moles of ice are melted by 13.4 kJ of energy?)
x = 2.23 mol (2.23 mol of ice melted by 13.4 kJ of energy)
What's next?
2 answers
Yes, 2.23 mols ice are melted? How many grms is that? grams = mols x molar mass = approx 40 g. How much ice did you have? That's 1,000 g. How much ice is left. Approx 1000-40 = ?
Question text
Calculate the energy required to melt 21 g of ice at 0 oC.
The molar heat of fusion for ice is 6.02 kJ/mol.
Answer kJ
Calculate the energy required to melt 21 g of ice at 0 oC.
The molar heat of fusion for ice is 6.02 kJ/mol.
Answer kJ
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