(a) Interpretation: The species with higher boiling point in the pair C 7 H 1 6 or C 1 0 H 2 2 needs to be determined. Concept introduction: Boiling point of a liquid depends on the strength of the intermolecular forces. When the intermolecular forces are high, boiling point of the liquid is also high.
(a) Interpretation: The species with higher boiling point in the pair C 7 H 1 6 or C 1 0 H 2 2 needs to be determined. Concept introduction: Boiling point of a liquid depends on the strength of the intermolecular forces. When the intermolecular forces are high, boiling point of the liquid is also high.
Solution Summary: The author explains that the species with higher boiling point in the pair C 7 H 1 6 or C 1 0 H 2 2 needs to be determined.
The species with higher boiling point in the pair C7H16or C10H22needs to be determined.
Concept introduction:
Boiling point of a liquid depends on the strength of the intermolecular forces. When the intermolecular forces are high, boiling point of the liquid is also high.
Interpretation Introduction
(b)
Interpretation:
The species with higher boiling point in the pair C3H8 and (CH3)2O needs to be determined.
Concept introduction:
Boiling point of a liquid depends on the strength of the intermolecular forces. When the intermolecular forces are high, boiling point of the liquid is also high.
Interpretation Introduction
(c)
Interpretation:
The species with higher boiling point in the pair CH3CH2SH and CH3CH2OH needs to be determined.
Concept introduction:
Boiling point of a liquid depends on the strength of the intermolecular forces. When the intermolecular forces are high, boiling point of the liquid is also high.
Based on the type or types of intermolecular forces, predictthe substance in each pair that has the higher boiling point:(a) propane (C3H8) or n-butane (C4H10), (b) diethyl ether(CH3CH2OCH2CH3) or 1-butanol (CH3CH2CH2CH2OH),(c) sulfur dioxide (SO2) or sulfur trioxide (SO3), (d) phosgene(Cl2CO) or formaldehyde (H2CO).
Consider a series of compounds: Methane (CH3), Ethane (CH3 CH3), Propane (CH3 CH2 CH3), Butane (CH3 CH2 CH2 CH3), and Pentane (CH3 CH2 CH2 CH2 CH3). For each compound (a) Indicate whether its molecules are polar or non polar. (b) Indicate predominant type of intermolecular forces in the liquid state. (c) Calculate the molar mass. (d) Convert each boiling point from Celsius degrees to Kelvins. (e) Plot a graph of boiling point (in K) versus molar mass. (f) Show the relationship between molar mass and boiling point?
Which of the following compounds exhibit London dispersion forces: (a) NH 3; (b) H 2O; (c) HCl; (d) ethane (C 2H 6)?