Question

How much heat does it take to melt 5.0g solid copper?

Answer 1

`Q=1.04kJ`

Step-by-step explanation:

Hello,

In this case, for latent heat (phase change) we need to consider the enthalpy associated with the involved process, here, melting or fusion; thus, the enthalpy of fusion of copper is 13.2 kJ/mol, therefore, the heat is computed as:

`Q=m\Delta H_(fus)`

Nevertheless, since the given enthalpy is per mole of copper, we need to use its atomic mass to perform the correct calculation as follows:

`Q=5.0g*(1mol)/(63.54)* 13.2(kJ)/(mol)\\ \\Q=1.04kJ`

Which is positive as it needs to be supplied to the system.

Best regards.