Chem Lect 2
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0o C and 1 atm are a part of ___________
standard temperature and pressure (STP)
This is the distance traveled by a gas molecule between collisions. Usually very very small distances.
the mean free path
Name the four characteristics of ideal gas that is not shared by real gas
- 1. Gas molecules have zero volume
- 2. Gas molecules exert no force other than repulsive force due to collisions
- 3. Gas molecules make completely elastic collisions.
- 4. the average kinetic energy of gas molecules is directly proportional to the temperature of the gas
Formula and units for the ideal gas law
- P= pressure (atm)
- V= volume (L)
- n= moles (mol)
- R=universal gas constant (0.08206 L*atm*K-1*mol-1) or (8.314 J K-1 mol-1)
- T=temperture (K)
At STP, one mole of any gas will occupy the standard molar volume of ________ liters
The amount of pressure contributed by any gas in a gaseous mixture is called this type of pressure of that gas.
To find it U must take the total pressure and multiply it by the mole fraction of the particular gas
Equation for Partial Pressure
Dalton's Law formula of partial pressure
How to find the average translational kinetic energy
Graham's law shows a relationship that gives the ratio of the rms velocity of tow gases in a homogeneous mixture. what is the formula?
V1/V2 = rootm2/rootm1
The spreading of gas from high pressure to very low pressure through a "pinhole"
This law gives information about the rates of two types of gaseous spreading : effusion and diffusion.
formula for effusion and mass of the gases
(effusion rate1)/(effusion rate2) = (root M2)/(root M1)
This is the spreading of one gas into another gas or into empty space
The higher the temperature the more collision can occur. More collisions equal higher chance of the reaction occurring. This leads us to believe:
The rate of a reaction increases with temperature
This provides an enlightening method for visualizing chemical reactions. In order for a chemical reaction to occur, the reacting molecules must collide. There are a high frequency of collisions but they do not always result in a reaction.
The collision model of reactions
The threshold energy that must be reached by the relative kinetic energies of the colliding molecules in order to a reaction to occur
These are species that are products of one reaction and reactants of a later reaction in a reaction chain. Their concentration is often very low because they are often unstable and react as quickly as they are formed
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