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

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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.

User Ruben Marin
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