Shared Flashcard Set

Details

Gas Laws
concepts and formulas
15
Chemistry
Undergraduate 1
01/17/2013

Additional Chemistry Flashcards

 


 

Cards

Term

For gas laws

what is the unit for

1.volume

2. temp

Definition

1. L or ml

2.K

Term
give formula for average molecular speed of a gas
Definition

KE= 1/2 mv2

= 3/2 kT

Term
give the formula for root mean square speed
Definition

urms=√3RT/M

R=8.325 J/K.mol

Mass = kg/mol

T = must be converted to Kelvin

Term
what is Graham's law?
Definition

based on:

heavier gases diffuse more slowly than lighter gases b/c of their differing average speeds.

Graham: the rates of gases at which gas diffuse are inversely proportional to the square root of their molar masses.

Term
formula for graham's law
Definition
r1 /r2 =√M2/ M1
Term

which gas will move faster:

Gas A:  mass 1kg at 20k

Gas B: mass 3kg at 5K

 

Definition

gas A 

b/c it at a higher temp

smaller size

Term
Write ideal gas law including units
Definition

PV=nRT

P=atm

V= L

n=mol

R=8.315 J (K.mol)/ 0.0821 (L* atm)

T=K

 

Term
Rearrange the ideal law to find changes in temp,pressure,volume, where moles is held constant
Definition

P1V1  =     P2V2

T1      T2

Term

Rearrange the ideal law to solve for V2 , where  temp ,pressure have a before and after value

(moles are held constant)

Definition
V2=V1 (P1/ P2) (T1 / T2)
Term
Formula how to calculate the molar mass of a gas using the density of a gas at STP
Definition

M=dstp/ 22.4stp

 

=

where vol is 22.4

d= density

Term

How do real gases behave during changes  in pressure?

extremly high pressure?

Definition

as pressure rises:

particles come closer & condense into liquid

 

extremly high pressure:

gas's volume becomes bigger

Term
How do real gases behave during decreases    in temp? (2)
Definition

as temp decrease: 

gas condense into a liquid state

volume decreases

Term
what is the  name of the equation that is used when a gas  doesnt follow gas laws?
Definition
van der waals
Term
write the van der waals equation
Definition

(P + n2 a )   (V-nb)  

V2

 

= nRT

Term

If the molar mass of gas is increased, what occurs? 

Is this behavior ideal?

Definition

↑ molecular mass=↑ collisions

= ↑ interactions

↑less ideal

 

Supporting users have an ad free experience!