Unit 6- The Gaseous State Flashcards

1
Q

solid

A

has fixed shape and volume
units: g/cm^3 or g/mL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

liquid

A

has fixed volume but no definite shape
unit: g/mL

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

gas

A

has no fixed volume or def shape
unit: g/L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

pressure

A

force per unit area exerted on a surface
unit: 1Pa = 1kg/ ms^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

barometer

A

used to measure pressure of atmos
- height(h) = 760mm at normal atmos pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

manometers

A

both open and closed end manometers measure pressure diffs
- pg>pa (h=pg-pa)
- pg<pa (h=pa-pg)
- h=pg

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Boyle’s Law

A

V = k x 1/p
PV = K (if T and n are same)
*P1V1 = P2V2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Charles’ Law

A

V = k2 x T
0K = -273.15C
T in kelvin
*V1/T1 = V2/T2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Avogadro’s Law

A

V= k3 x n(mol)
*V1/n1 = V2/n2 (const T and P)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Ideal Gas Law

A

PV=nRT
R= 0.08206 Latm/molK
- vol of 1 mol at STP (T=0C P=1atm) = 22.4L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

MM

A

(mass x R x T) / (P xV)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Density

A

(MM x P) / (R x T)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

coeff

A

= L w/ const temp and pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Dalton’s Law of Partial Pressures

A

Pt=Pa+Pb

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

mole fraction (x, chi)

A

the # of mol of 1 component of a mix divided by the total # of mols of all substances present in the mix

Xa= na/ na + nb +nc…

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Partial Pressure

A

Pa = Xa x Pt

17
Q

Collecting gas over water

A

Pg = Pt - Ph2o

18
Q

Kinetic Molec Theory of Gases

A

1) No forces of attraction or repulsion between gas particles
2) size of gas particles can be negligible
3) No loss in KE occurs when gas particles collide
4) KE changes only if T changes

19
Q

Avg speed

A
  • called the root mean square (rms) speed, Urms
  • the square root of the avg squared speed
20
Q

Urms =

A

sqaure root of (3RT/ MM)
*R= 8.314 kgm^2/s^2molK
- MM= kg/mol

21
Q

Effusion

A

the passage of gas through a small hole into an evacuated space
* gases with low MM effuse more rapidly

22
Q

diffusion

A

the mixing of particles due to motion

23
Q

Graham’s Law of Effusion

A

relative rates of effusion can be used to determine MM (M)

rate of effusion A/ rate of effusion B = square root of (Mb/Ma)

24
Q

Graham’s law when equal vol or pressure of gas A and B are used

A

effusion time (t)

tb/ ta = square root of (Mb/ Ma)

25
Q

deviations from Ideal Behavior

A

at high pressures:
- ideal gas law fails
- kinetic molec theory fails (forces of attraction)
- assumption gas particles are small compared to distances between them fails

26
Q

Van der Waals Equation

A

corrects for attractive forces and vol occupied by gas molec

(P + an^2/v^2)(V-nb) = nRT
- a = const relat to strenght of attraction forces
- b = const that depends on the size of the gas particles