If 756 J of heat is needed to melt 12g of gold, what is the heat of fusion?

Question

asked Mar 5, 2021 168k views

1 Answer

Ruben Marin · Answer 1 · 2021-03-12T18:04:39+0000

Answer:

$\Delta _mH=63J/g$

Or:

$\Delta _mH=12.4kJ/mol$

Step-by-step explanation:

Hello,

In this case, since the required heat to turn solid gold into liquid gold is computed by:

$Q=m\Delta _mH$

Which is mass and enthalpy of fusion- dependent, we compute the enthalpy of fusion as shown below:

$\Delta _mH=(Q)/(m) =(756J)/(12g)\\ \\\Delta _mH=63(J)/(g)$

Or in kJ/mol (typical data):

$Delta _mH=63(J)/(g)*(1kJ)/(1000J) *(197g)/(1mol)\\ \\Delta _mH=12.4kJ/mol$

Best regards.