Gaseous State Flashcards
Which law gives the relationship between Volume and Temp at constant pressure
Gay-Lussac
State Boyle’s law
P is directly prop. to V at const. T
State Avogardo’s law
At constant T and P,equal volumes of any gas contain equal number of moles
In the ideal gas equation,R has different values wrt difference units used. Write each of them
R=0.0821 L atm/K mol
=8.314 J/K mol
=2 cal/K mol
State Dalton’s law of partial pressure
If there are 2 or more gases in a container of fixed volume,that are non-reactive with each other.Then,pressure exerted by each gas is equivalent to the case where the same volume of gas is solely present in the exact same container.
Difference between effusion and diffusion?
https://courses.lumenlearning.com/boundless-chemistry/chapter/diffusion-and-effusion/
Kinetic energy formula
PV=1/3mnc^2
what does m,n and c indicate in the KE formula indicate?
m-> mass of one molecule
n->no. of molecules
c-> root mean square velocity
What is the Boltzmann constant?Give it’s formula
K=R/No
No-> avogardo’s constant
Formula for:
1) Vrms
2) Vmps
3) Vavg
1) sqrt(3RT/M)
2) sqrt(8RT/3.14M)
3) sqrt(2RT/M)
Which out of the 3 speeds is the highest? Also:
Vmps:Vavg:Vrms=?
(asked in JEE Adv. 2020)
Vrms
1:1.128:1.224
What happens if we increase the temperature and observe the gases’ maxwell distribution curve graph?
Explain in regards to change in fraction of molecules moving with a) Vmps b) a certain value of kinetic energy
What causes the changes?
The curve will flatten out. Fraction of molecules moving with Vmps decreases as the movement is more random. Overall the energy will increase,but fraction of molecules moving with particular energy values will decrease
Define Z,compressibility factor
Z=Molar volume(real)/Molar Volume(ideal)
If Z<1->
Gas is more compressible
Z>1–>
Gas occupies larger volume than ideal
