How many grams of ice at 0 oC and 1 atm could be melted by the addition of 2.2 kJ of heat? The ∆Hfus of ice is 6.0 kJ/mol.
kJ heat added = mass ice x heat fusion.
Then convert moles ice to grams. g = mols x molar mass
To solve this problem, we need to use the concept of moles and the heat of fusion (∆Hfus) of ice.
1. Calculate the number of moles of energy supplied:
We have the given amount of heat, which is 2.2 kJ (kilojoules). To convert this to joules, multiply by 1000: 2.2 kJ * 1000 = 2200 J.
We also know that the molar enthalpy of fusion (∆Hfus) of ice is 6.0 kJ/mol. Since 1 kJ is equivalent to 1000 J, the ∆Hfus of ice is 6.0 * 1000 J/mol = 6000 J/mol.
To find the number of moles of energy supplied, divide the energy by the ∆Hfus:
Moles of energy = (2200 J) / (6000 J/mol) = 0.367 mol
2. Calculate the mass of ice using the molar mass:
The molar mass of water (H2O) is approximately 18.02 g/mol.
Since the molecular formula of ice (solid water) is also H2O, the molar mass of ice is also 18.02 g/mol.
To find the mass of ice, multiply the number of moles by the molar mass:
Mass of ice = (0.367 mol) * (18.02 g/mol) = 6.56 g
Therefore, 2.2 kJ of heat can melt approximately 6.56 grams of ice at 0 oC and 1 atm.