Gas Lawz Flashcards
(20 cards)
Pressure
P= force/area; collision frequency occurs on the microscopic level.
Collision Frequency
Collision frequency= rate at which collisions occur; increases with increased temp, increased [gas], increased pressure, decreased volume
Collision force
the force exerted by a gas during a collision (aka an impulse)
Mean Free Path
How far a particle will move before it collides with another particle (microscopic to volume)
Average Kinetic Energy
Mean energy of a particle in a system (microscopic to temperature)
R value
R = 0.0821 (L * atm / mol * K)
4 Assumptions for the Kinetic Molecular Theory of Gases
1) Particles have a negligible volume
2) All collision are perfectly elastic
3) Particles are in random translational motion
4) Particles exert no IMF
Gases are most ideal when…
1) at high temperature (you need enough energy to overcome IMF)
2) at low pressure (because you have minimal interactions at low pressure)
Boyle’s Law
At constant T:
P1 V1 = P2 V2
Charle’s Law
At constant P:
V1/T1 = V2/T2
Avocado’s Law
At constant P and T:
P1/n1 = P2/n2
Deviations of Ideal Gas Law
1) Deviations due to Pressure
2) Deviations due to Volume
Result: Van Der Waals Eq
Deviation due to Pressure EQ
Pressure ideal = Pressure observed + (a)(n)^2 / v^2
Deviation due to Volume EQ
Volume ideal= Volume Container - (n * b)
Combined Van Der Waals EQ
(Pobserved + an^2/v^2) (Vcontainer - nb) = nRT
a= attractive coefficient b= bigness coefficient
Partial Pressure
= (mole fraction) (total pressure)
Mole Fraction
= # of moles/ total moles
of stereoisomers
= 2^n where n= # of chiral centers
Steps of Free Radical Bromination
1) Initiation
2) Propagation (Br abstracts most substituted hydrogen on the molecule)
3) Termination
RXN: alkane –> pdt (reagent: Br2 –> hv)
Chair conformation
Staggered vs Eclipsed
Anti vs Gauche
