Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1809 K), given that: ?Hfus = 13.80 kJ/mol.
Mass of iron = 2.00 kg = 2000 g
Moles of iron = mass/molar mass
= 2000/55.847 = 35.812 mol
Heat needed = moles x ΔHfus
= 35.812 x 13.80
= 494.2 kJ
Energy needed to change phase is q = moles of substance * heat of fusion
2000 g iron/55.85 g/mol = 35.8 mol iron
Heat of fusion for iron = 13.8 kJ/mol
35.8 mol * 13.8 kJ/mol = 494.1 kJ
Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1809 K), given...
Calculate the amount of heat needed to melt 2.00 kg of iron at its melting point (1809 K), given that: ?Hfus = 13.80 kJ/mol.
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