Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

CH0002 > Gas Kinetics > Flashcards

Gas Kinetics Flashcards

1
Q

What is Boyle’s Law

A

At constant temperature, for a given sample of gas, the volume is inversely proportional to the pressure

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

What is the mathematical representation of Boyle’s Law

A

Volume is proportional to 1/P
Volume = constant/ pressure
PV= constant
P1 x V1 = P2 x V2

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

If a flask containing an ideal gas at a pressure of 5atm is connected to a second flask of volume 300cm3 the pressure drops to 3atm. What was the volume of the first flask

A 
P1V1=P2V2
5xV1 = 3x(300+V1)
5V1= 3V1 + 900
2V1 = 900
V1 = 900/ 2
V1 = 450cm3
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is Charles’ Law

A

The volume of a given sample of gas at constant pressure is proportional to temperature

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

What is the mathematical representation of Charles’ Law

A

Volume is proportional to temperature

V1/ T1 = V2/ T2

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

What is Avagadro’s principle

A

The volume of a sample of gas at a given temperature is proportional to the number of gas molecules in the sample

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

What is the mathematical representation of Avagadro’s principle

A

Volume is proportional to number of moles (independent of which gas it is)
Volume = constant x n

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

What is the volume occupied by 1 mole of gas

A

22.4dm-3

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

Calculate the volume occupied by 10g CO2

A

No moles of CO2 x 22.4L per mole
10/44 x 22.4/1
5.2 L

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

What is the ideal gas law

A

PV = nRT

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

What is R and what is its value

A

R is the gas constant

R = 8.314 JK-1mol-1

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

What are the 3 assumptions of the ideal gas law

A
  1. ) gases consist of small particles which have negligible volume
  2. ) gas molecules are in constant rapid motion, undergoing elastic collisions with each other and their container (energy is conserved)
  3. ) molecules do not interact with each other except during collisions
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Give experimental evidence for the ideal gas assumptions

A
  1. ) compressibility of gases
  2. ) Brownian motion
  3. ) gases expand to fill their container
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Give experimental evidence against ideal gas assumptions

A

1) molecules have a finite mass

2) attractive interactions exists between molecules as: measured pressure

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

Describe experimental evidence that shows:

Measured pressure

A

Pressure due to collisions within container walls.
Attractive dispersion forces exist between molecules.
Molecules near walls attracted to those in bulk
Pmeasured

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

Why is volume of gas not negligible at high pressure

A

Vreal > Videal
For an ideal gas PV/RT = 1
At high pressures PV/RT > 1

17
Q

Describe the deviation that occurs at moderate pressure

A

A negative deviation occurs due to attractive dispersion forces

18
Q

What is the distribution of energies

A

The average kinetic energy of particles within a gas depends on the temperature, but there is a distribution of kinetic energies amongst the gas particles

19
Q

What does the Zartman experiment show

A

That particles travel at different speed due to them hitting different sections of the second disk. Also temperature affects the speed at which particles travel

20
Q

What is Maxwell-Boltzmann distribution

A

As temperature increases, the distribution broadens (wider range) and shifts (right) to faster average speeds

21
Q

What is diffusion

A

The mixing of atoms of different types

22
Q

What is effusion

A

The escape of a gas through a small hole

23
Q

What is Graham’s law of effusion

A

At a given pressure and temperature the rate of effusion of a gas is inversely proportional to the square root of the molecular mass

24
Q

What equation based on Graham’s law is used in effusion calculations

A

Rate of effusion of gas 1 = rate of effusion of gas 2

√(M2/M1)

25
Q

Which of hydrogen and carbon dioxide will effusion faster and by how much

A

Rate of effusion of H2/ rate of effusion of CO2
√(44/2) = 4.7
So H2 effuses approximately 5x as fast as CO2

26
Q

The rate of effusion of C2F4 is 4.6x10-6 mol hour-1. An unknown gas containing F, N, O diffuses at a rate of 6.5x10-6 mol hour-1. Deduce the formula of an unknown ga

A 
Effusion gas 1/ effusion gas 2 = √M2/M1
= 6.5x10-6/ 4.6x10-6 = √100/M1
= 1.4squared = 100/M1
= 1.9 x M1 = 100
M1 = 100/1.9 
=50
Mr = 50
F= 19, N=14, O=16 sum= 49
Gas = NOF

CH0002 (13 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions