Which of the following best explains why more energy is required for the process occurring at 110 K than for the process occurring at 90 K? A. Intermolecular attractions are completely overcome during vaporization B. Intermolecular attractions in the solid phase are weaker than in the liquid phaseC. Electron clouds of methane molecules are less polarizable at lower temperaturesD. Vaporization involves larger increase in temperature

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acarr7841 acarr7841

05-12-2022
Chemistry

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Which of the following best explains why more energy is required for the process occurring at 110 K than for the process occurring at 90 K? A. Intermolecular attractions are completely overcome during vaporization B. Intermolecular attractions in the solid phase are weaker than in the liquid phaseC. Electron clouds of methane molecules are less polarizable at lower temperaturesD. Vaporization involves larger increase in temperature

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NehaKumari123 NehaKumari123 · Answer 1 · 2022-12-08T07:54:12+01:00

Vaporization totally overcomes intermolecular attractions. Water has an enthalpy of vaporization (energy required to boil) of 40.7 kJ/mol.

A is the ideal answer.

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