Chapter 6 Flashcards
(21 cards)
Melting Point
The temperature at which a solid become a liquid.
Boiling Point
The temperature at which a liquid becomes a gas
Dipole-dipole forces
Polar molecules whose opposite charged ends attract one another
Like a magnet
Solute
A substance dissolved in a solvent
Solvent
Whatever is dissolving the solute
Molarity
Moles of solute per liter of a solution.
M= mol/liter
Boyle’s Law
At constant temperature, the volume of a gas is inversely proportional to its pressure.
When pressure goes up, the volume goes down
Charles’ Law
At constant pressure, the volume of a gas is directly proportional to its absolute temperature.
Combined gas Law
PV/T= PV/T
1 2
Ideal gas Law
PV= nRT
R= 0.0821 L(atm)/ mol(K)
Steps in a stoichiometric calculation
- Balance equation
- Molar mass
- Stoichiometry
- Use ,Olaf mass to find the mass of desired substance
Vaporization
The conversion of a liquid to a gas
Condensation
The conversion of a gas to a liquid
Sublimation
A conversion from a solid state directly to a gaseous state
Dispersion forces
Momentary, weak, attractive forces between molecules
Hydrogen bond
A strong bond that has positive end that is a H attached to N, O, or F and the negative end is a second N, O, or F atom
Solution
A homogeneous mixture of two or more substances
Kinetic- molecular theory
The theory in which gases are explained. That is:
- They move more rapidly and constantly and in straight lines
- The are far apart
- There is little interaction among them
- When they collide, energy is conserved
- Temperature is a measure of their average kinetic energy
Molar volume
The volume occupied by 1 mol of the gas
Standard temperature and pressure
At 0 degrees C ;and 1 atm, the molar volume is 22.4 L for any gas
Avogadro’s Law
The volume of all gases measured at the same temperature and pressure contain the same number of molecules.
