Vocabulary (Ch 10)
Another word for intermolecular forces
Van der Waals forces
As kinetic energy increases, what happens to IMFs?
decrease
The simplest, repeating unit in a solid is its
Unit cell
NaCl (s) + H2O (l) →Na+ (aq) + Cl– (aq) + H2O (l)
What is the expected van't hoff factor?
2
(moles of particles in solution/ moles of formula units dissolved)
This is the part of a solution that is present in the largest concentration
solvent
Strong attractive forces between atoms in a molecule
intramolecular forces
As surface area increases, what happens to IMFs?
increase
As temperature increases, what happens to the solubility of gases in liquids?
decreases
Water vapor has a vapor pressure of 23.8 mmHg at 25˚C and a heat of vaporization of 40.657 kJ mol–1. What is the vapor pressure (to one decimal place in mmHg) of water at 92˚C?
482.5 mmHg
Substances that produce ions when dissolved in water
ions
Weakest intermolecular force
Dispersion forces
As surface area decreases, what happens to energy?
decreases
This equation describes the quantitative relation between a substance’s vaporpressure and its temperature
Clausius-Clapeyron equation
How much heat is required (in kJ mol–1 to two decimal places) to vaporize one mole of a compound that has a measured vapor pressure of 0.032 atm at 0oC and 0.178 atm at 52oC?
24.37 kJ mol–1
colligative properties
Resistance of a liquid to flow
viscosity
Higher rate of vaporization occurs with (larger or smaller) surface area?
higher
As pressure increases, what happens to the solubility of gasses in liquids?
increases
How much heat (in kJ to nearest whole number) is required to convert 500 g of ice at –30˚C into steam at 150˚C (at sea level)?
∆Hfus= 6.01 kJ/mol ∆Hvap= 40.67 kJ/mol
C ice= 2.09 J/g˚C; C water= 4.18 J/g˚C
C steam= 1.84 J/g˚C
1,582 kJ
solution that contains more than the equilibrium amount of solute
supersaturated
Ability of a liquid to flow against gravity in narrow spaces
capillary action
Rank the following from strongest to weakest:
dipole/dipole, dispersion, ionic, H-bonding
Ionic > H-bonding > dipole/dipole > dispersion
Write the equation for Henry's Law
Sgas = kH Pgas
The vapor pressure of 1-propanol is 10.0 torr at 14.7 °C. Calculate the vapor pressure at 52.8 °C.
Given:
Heat of vaporization of 1-propanol = 47.2 kJ/mol
100.2 torr.
A sealed can has higher P, increasing the solubility of CO2
This is quanitfied by what equation?
Henry's law