150 130 120 110 100 ???,-8.2 klinol vap AHs 094 kJ/mol 80 70 60 - 50 40 30 20 10
ID: 1036198 • Letter: 1
Question
150 130 120 110 100 ???,-8.2 klinol vap AHs 094 kJ/mol 80 70 60 - 50 40 30 20 10 E Heat Added energy is required to melt 64 g 41. The enthalpy of vaporization of water is molar mass of 40.7 kJ/mol. Which of the following best explains why the enthalpy of vaporization of methane is less than that of water? kJ (A) Methane does not exhibit hydrogen bonding, but water does. (B) Methane has weaker dispersion forces. (C) Methane has a smaller molar mass. (D) Methane has a much lower density he follo best explains why more equireMor the process occurrinkat for the nrocess occurrino at 0Explanation / Answer
Amount of energy required to transform a quantity of substance from liquid to gas is called as the enthalpy of vaporization.
Heat is absorbed when a liquid boils because molecules which are held together by mutual attraction in the liquid are set to free of each other as liquid is transformed into gas. Such a separation requires energy. In general the energy needed differs from one liquid to another depending on the magnitude of the intermolecular forces. We can thus expect liquids with strong intermolecular forces to have larger enthalpies of vaporization. And hence Water exhibit strong hydrogen bonding where as it is absent in Methane. This makes less energy is required to vaporize certain amount of methane to gas as compared to water. So, water has high enthalpy of vaporization than methan.
Answer is option A.
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.