Describe how van der Waals bonds contribute to the functionality of adhesives, surfactants, and emulsifiers. What are the practical applications of these bonds in consumer products?
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Describe how van der Waals bonds contribute to the functionality of adhesives, surfactants, and emulsifiers. What are the practical applications of these bonds in consumer products?
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- The boiling point of ammonia (NH3) and phosphine (PH3) are 240K and 185K respectively. Account for this difference. Explain why Hydrogen gas exist as a diatomic molecule whereas Helium gas is monoatomic? Explain why Kerosene readily dissolves in petrol but not in waterIn designing an effective drug, pharmaceutical scientists oftenintentionally introduce fluorine in order to alter the drug’s chemical orbiological properties without significantly altering its shape. Discuss theimportance of this alteration using the chemical structure of Prozac(Fluoxetine)Briefly describe the physical origin of the van der Waals bond. Name some elemental systems in which this type of bond is dominant.
- Describe the classification of polymers on the basis of their molecular structure. Give an example of each class.What is hydrophobic effect? What is its significance in biomolecular structure?Using the bond breaking and bond forming method, estimate the enthalpy associated with combusting one mole of hydrogen with molecular oxygen to form water under standard conditions (1 M, 1 atm, 298 K).
- briefly explain why the oleic acid molecules organize themselves into a monolayer?A 0.325 g sample of a gaseous hydrocarbon (compound containing carbon and hydrogen only) occupies a volume of 193 mL at 749 mmHg and 26.1°C. Determine the molecular mass, and write a plausible Lewis structure for this hydrocarbon.In a hydrogen molecule, the two hydrogen atoms are held together by a single bond with a bond energy of 436 kJ/mol of hydrogen. In other words, to break the H-H bonds in one mole of molecular hydrogen requires the expenditure of 436 kJ of energy. Using the balanced chemical equation for the formation of water from oxygen and hydrogen (shown above), and interpreting the stoichiometric coefficients as mole amounts, how much energy must be expended in breaking the H-H bonds? kJ
