STPSTP=1atm,0degrees celsius
Standard Temperature and Pressure 
1 mol1mol=6.02x10^23particles X=molar mass(g) X
particles {
atoms(single elements),
molecules(two or more non metals),
formulas units(two or more non metals)(f.u)
ions(minerals, electrolytes,charged particles
} 
Conversion: inch to mm1in=2.54cm  100cm=1m  1m=1,000mm 
Conversion: atm to mmHg1atm=kPa=760torr=10.3mH2O=14.7psi=760mmHg 
Things to know about mols1mol=6.02x10^{23}particles  1mol=22.4L (only for gases) 
  Rules for Sig FigsTo determine the number of significant figures in a number use the following 3 rules:
1.Nonzero digits are always significant
2.Any zeros between two significant digits are significant
3.A final zero or trailing zeros in the decimal portion ONLY are significant
Example: .500 or .632000 the zeros are significant
.006 or .000968 the zeros are NOT significant
For addition and subtraction use the following rules:
1.Count the number of significant figures in the decimal portion ONLY of each number in the problem
2.Add or subtract in the normal fashion
3.Your final answer may have no more significant figures to the right of the decimal than the LEAST number of significant figures in any number in the problem.
For multiplication and division use the following rule:
1.The LEAST number of significant figures in any number of the problem determines the number of significant figures in the answer. (You are now looking at the entire number, not just the decimal portion)
This means you have to be able to recognize significant figures in order to use this rule
Example: 5.26 has 3 significant figures
6.1 has 2 significant figures 
No think math method? for conversion#unit^{1} x #unit(converting to) / #unit^{1}
#=number
cancel like units
then multiple and divide then you get your answer with new units 
AbbreviationsAtmosphereatm
BarBar
millimeter of mercurymmHg
Pascalpa
Pounds per square inchpsi
Torrtorr 
 
The 7 Diatomic ElementsHydrogen (H2)
Nitrogen (N2)
Oxygen (O2)
Fluorine (F2)
Chlorine (Cl2)
Iodine (I2)
Bromine (Br2) 
Useful things to know about gases1. Gas particles are much farther apart from each other than liquid and solid particles
2. Gases are fluids, fluids are any substance that can flow
3. Gases have low density
4. Gases are highly compressible
5. Gases completely fill a container
6. Kinetic molecular theory
*model used to predict gas behavior
*constant random motion, increasing temp, increases motion
7. Intermolecular forces(attractive forces) are very weak or nonexistent between gas particles 
  Combined gas LawP^{1}V^{1}/T^{1}=P^{2}V^{2}/T^{2}
The Combined Gas Law is useful when: Given two pressures, volumes, or temperatures and asked for an unknown pressure, volume, or temp. Whenever it gives you conditions for one gas, and asks for conditions of another gas, you're most likely going to use this Law. 
Charle's lawv^{1}/t^{1} = v^{2}/t^{2}
Since pressure is kept constant, the only variable that is manipulated is temperature. This means that we can use Charles's law in order to compare volume and temperature. Since volume and temperature are on opposite sides of the ideal gas law, they are directly proportional to one another. 
Ideal gas LawPV/nT=nRT/nT
P=atm
V=L
n=# of mols
T=Kelvin
R= 0.0821 atm x L / mol x K Always divide the numbers underneath 
Boyles lawP^{1}V^{1} = P^{2}V^{2}
Key Points:
~According to Boyle’s Law, an inverse relationship exists between pressure and volume.
~Boyle’s Law holds true only if the number of molecules (n) and the temperature (T) are both constant.
~Boyle’s Law is used to predict the result of introducing a change in volume and pressure only, and only to the initial state of a fixed quantity of gas.
~The relationship for Boyle’s Law can be expressed as follows: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume values, and P2 and V2 are the values of the pressure and volume of the gas after change. 
Ideal gas LawPV/nT=nRT/nT
P=atm
V=L
n=# of mols
T=Kelvin
R= 0.0821 atm x L / mol x K Always divide the numbers underneath 
Gaylusacs lawp^{1}/t^{1} = p^{2}/t^{2}
GayLussac's law is a form of the ideal gas law in which gas volume is kept constant.
When volume is held constant, pressure of a gas is directly proportional to its temperature.
The usual equations for GayLussac's law are P/T = constant or Pi/Ti = Pf/Tf. 

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