The order of solubility is as follows
CCl4 > CHCl3 > NaCl
More the electronegative atom such as chlorine more will be its solubility.
Using your knowledge of intermolecular forces, arrange the following chemicals according to their solubility in the...
5. Using your knowledge of intermolecular forces, explain the following observations: a. Rare gases and hydrogen assume liquid state at finite temperature. b. In the separation of aromatics from paraffins by extraction, liquid SO2 is a better solvent than liquid NHs. At 30°C, the solubilities of ethane and acetylene in n-octane are about the same. However, at the same temperature, the solubility of acetylene in c. dimethylformamide is very much larger than that of ethane. d. One of the main...
Using your knowledge of intermolecular forces, explain the following observation: a) At 300°C and 30 bat, the internal energy of water is less than at 300°C and 20 bar. b) At 300 K and 30 bar, the compressibility factor of isopropanol (H3CCOHCH3) is less than that of n-pentane (C3H12), but at 500 K and 30 bar, the compressibility factor of isopropanol is greater than that of n-pentane.
INTERMOLECULAR FORCES INTRODUCTION LEARNING OBJECTIVES To relate the effecet of intermolecular forces on relative melting points and vapour pressures of some organic substances THEORY Weak attractive forces that occur between individual molecules in substances are called intermolecular forces. These include London dispersion forces, dipole-dipole forces and hydrogen-bonding forces. Collectively, the three types of intermolecular forces are referred to as Van der Waals forces. These attractive forces are much weaker than the chemical bonds between atoms in a molecule. Note that...
In which of the following substances are intermolecular forces of attraction absent? A) HF(l) B) CCl4(l) C) NaCl(l) D) H2O(l) E) N2(l)
2. Use your knowledge of intermolecular forces to provide an explanation for why the boiling point of 2-hexanol is higher than the boiling point of 2,3-dimethyl-2-butanol. Be sure to consider all intermolecular forces in the molecules.
2. Use your knowledge of intermolecular forces to provide an explanation for why the boiling point of 2-hexanol is higher than the boiling point of 2,3-dimethyl-2-butanol. Be sure to consider all intermolecular forces in the molecules.
Chapter 9 - Solution Formation, Solubility, Miscibility 34. Based on the predominant intermolecular forces, indicate whether or not each of the following pairs of compounds are likely to form a solution? a. H2SO04 and H20 b. CsH18 and CeH6 C. CH2Cl2 and H2O d. CS2 and CCl4 e. C6H14 and H20 f. CO2 and H2O g. NaCI and H2O
10. (14 pts) For the compounds below: a. Identify the strongest intermolecular force present in each molecule. b. Arrange the following molecules in order of lowest vapor pressure to highest vapor pressure. c. Briefly justify your answer to part b using your knowledge of intermolecular forces. Molecule * HH * Strongest Intermolecular Force: Lowest vapor pressure: < < Highest vapor pressure 11.(12 pts) Ethanol (CH-OH, FW-46.08 g/mol) melts at -114 °C and boils at 78 °C. How much heat is...
arrange the following molecules according to tje strength of
their dispersion forces
DO Question 3 Arrange the following molecules according to the strength of their dispersion forces. For this question, 1 - Largest dispersion force and 6 - Smallest dispersione сн. Structure 1 CH-CH-C-CH-CH, Structure 4 CHE CH, CH, Structure 2 CH-CH2-CH2-CH2-CHA Structure 5 CH-CH2-CH2-CH-CH-CH-CH, CH, сн. Structure 3 CH-C-CH, Structure 6 CH, CH, CH, CH, Structure 1 Choose Structure 2 Choose Structure 3 Choose Structure Choose Structures [Choose Structure...
Which of the following best describes London dispersion forces. Question 1 options: the intermolecular forces that exist when ions from an ionic compound are attracted to the dipole of polar molecules in a mixture. involves molecular orientations in which the positive end of one dipole is near the negative end of another forces that exist only between molecules that contain hydrogen atoms bonded to highly electronegative atoms such as O, N, F. Interactions between temporary dipoles cause atoms to be...