Question | Answer |
Boyle's Law | the pressure and volume of a gas are inversely proportional when the temperature and number of moles remain constant |
equation for boyle's law | P1V1=P2V2 |
charles's law | the volume and temperature of a gas are directly proportional when the pressure and number of moles remain constant |
equation for charles's law | V1/T1=V2/T2 |
Dalton's Law of partial pressures | Ptotal=P1+P2+P3... |
partial pressure | the pressure of a single gas in a mixture as if that gas alone occupied the container |
how to find partial pressure | (moles/total moles) x (Ptotal) |
Gay Lussac's Law | the pressure of a gas is directly proportional to the temperature when volume and # of moles remain constant. |
equation for Gay Lussac's law | P1/T1=P2/T2 |
what units of temperature do you ALWAYS use for these equations? | KELVIN! K=C+273. because of absolute zero |
the combined gas law combines which laws? | boyle's charles's, and gay lussac's law |
equation for the combined gas law | (P1V1)/T1=(P2V2)/T2 |
what are the cons of all the other individual's laws? | there were only 2 variables that were allowed to change, and the other 2 were held constant (unrealistic) |
what is the advantage of the combined gas law? | allows all 3 variables to change. the only constant is the amount of gas |
what is the purpose of the ideal gas law | allows you to calculate the amt of gas at any specified conditions |
equation for the ideal gas law | PV=nRT |
what does the variable P stand for? | P=pressure (atm) |
what does the variable V stand for? | V=volume (L) |
what does the variable n stand for? | moles |
what does the variable R stand for? | ideal gas constant (for atm, it's) 0.0821 |
what does the variable T stand for? | temperature (K) |
Ideal gas | a gas molecule that has no volume and no attractive forces |
real gas | a gas molecule that has volume and attractive forces; occurs at very low temperatures and high pressure |
characteristics of real gases | they convert into a liquid instead of compressing to 0 volume; van der Waals forces become significant due to the close proximity of the atoms |
Diffusion | The spontaneous spreading of particles throughout a given volume until they are uniformly distributed (perfume) |
effusion | The mvmt of gas through a small opening |
grahm's law equation (unimportant for the unit test) | v1/v2=√m2/√m1 |
grahm's law says that...? | small gases move faster than larger gases (molar mass) |