Question

calculate the amount of energy needed to melt 2.78 moles of iron at its melting point. ∆H did =13.807​

Answer 1

where q is the amount of energy required, n is the number of moles of the substance, and ∆H is the enthalpy of fusion (or melting) of the substance.
Substituting the given values, we get:
q = 2.78 moles x 13.807 J/mol
q = 38.36 J
Therefore, the amount of energy needed to melt 2.78 moles of iron at its melting point is 38.36 J.