Answer :

Final answer:

The heat required to completely melt 1.37 mol of isopropyl alcohol can be calculated using the enthalpy of fusion and the equation 'q = n * enthalpy of fusion'. However, the specific enthalpy of fusion for isopropyl alcohol is needed for an accurate calculation.

Explanation:

The question asks about the amount of heat needed to completely melt 1.37 mol of isopropyl alcohol at its melting point. For such computations, we typically use the concept of enthalpy of fusion, which is the amount of heat required to change one mole of a substance from the solid to the liquid state.

However, it is essential to know the specific enthalpy of fusion for isopropyl alcohol, which isn't provided in the question. An estimate, as seen with a substance such as ice, can be around 6.0 kJ/mol, but this could vary widely depending on the material.

In any case, once you know the enthalpy of fusion (let's denote it as Hfus), you can calculate the total heat (q) using the equation:

[tex]q= n * H_{fus}[/tex]

where 'n' is the number of moles, which is 1.37 in this example.

Learn more about Enthalpy of Fusion here:

https://brainly.com/question/32361849

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