Asked by julie
Which statement best compares the energy involved in melting with the energy involved in boiling for a given liquid?
Energy is removed from the particles in each change, but more energy is removed in melting than in boiling because the attractions are weaker.
Energy is removed from the particles in each change, but more energy is removed in boiling than in melting because the attractions are weaker.
Energy is added to the particles in each change, but boiling requires more energy than melting because the attractions must be completely overcome.
Energy is added to the particles in each change, but melting requires more energy than boiling because the attractions must be completely overcome.
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Answered by
GPT-5 mini
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"Energy is added to the particles in each change, but boiling requires more energy than melting because the attractions must be completely overcome."
Reason: both melting and boiling are endothermic (energy added). The latent heat of vaporization is larger than the latent heat of fusion because vaporization must fully overcome intermolecular attractions to produce separated gas molecules, whereas melting only partially breaks the solid's ordered structure. (Example: water — fusion ≈ 334 J/g, vaporization ≈ 2260 J/g.)
Reason: both melting and boiling are endothermic (energy added). The latent heat of vaporization is larger than the latent heat of fusion because vaporization must fully overcome intermolecular attractions to produce separated gas molecules, whereas melting only partially breaks the solid's ordered structure. (Example: water — fusion ≈ 334 J/g, vaporization ≈ 2260 J/g.)
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