Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > The Gaseous State > Flashcards

The Gaseous State Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is Avogadro’s Law?

A

For a gas at constant temperature and pressure, the volume of the gas is directly proportional to the number of moles of the gas.

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

What is the equation that can be deduced from Avogadro’s Law?

A

V1/n1 = V2/n2

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

What is the molar gas volume at s.t.p. and r.t.p.?

A

s. t.p. (10^5 Pa/1 bar and 273K): 22.7dm^3 mol^-1

r. t.p. (101325 Pa/1 atm and 293K): 24dm^3 mol^-1

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

What is Gay-Lussac’s Law?

A

For a fixed mass of gas at a constant volume, the pressure of gas is directly proportional to its absolute temperature.

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

What is the equation that can be deduced from Gay-Lussac’s Law?

A

p1/T1 = p2/T2

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

What is Charles’ Law?

A

For a fixed mass of gas at constant pressure, the volume of the gas is directly proportional to its absolute temperature.

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

What is the equation that can be deduced from Charles’ Law?

A

V1/T1 = V2/T2

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

What is Boyle’s Law?

A

For a fixed mass of gas at a constant temperature, the volume of gas is inversely proportional to its pressure.

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

What is the equation that can be deduced from Boyle’s Law?

A

p1V1 = p2V2

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

What is the ideal gas equation?

A

pV = nRT

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

What is the value of molar gas constant R?

A

8.31 J K^-1 mol^-1

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

What is the equation for the molar mass M of a gas?

A

M = mRT/pV

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

What is the equation for density of a gas?

A

ρ = pM/RT

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

What are the basic assumptions of the Kinetic Theory as applied to an ideal gas?

A
  1. An ideal gas consists of particles of negligible volume.
  2. The gas exerts negligible attractive forces on one another.
  3. The gas particles are in constant random motion.
  4. Collisions are perfectly elastic.
  5. The average kinetic energy of particles in agas is constant at a constant temperature and is proportional to the absolute temperature.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the two conditions for a real gas to approach ideality?

A

Low pressure: Gas particles are very far from each other, volume occupied by gas particles can be considered to have negligible volume compared to volume of the container. IMAF between widely spaced particles are negligible.

High temperature: Gas particles possess high KE to overcome IMAF, making IMAF negligible.

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

Why is negative deviation (pV/RT < 1) observed when pressure is moderately high?

A

The volume of the system is smaller. Gas particles are closer together and IMAF between the gas particles become more significant. The gas thus occupies a smaller volume than it would if it were ideal.

17
Q

Why is positive deviation (pV/RT > 1) observed when pressure is high?

A

The volume of the system is very small. Gas particles are so close together that there is repulsion between their electron clouds. This IMRF causes the gas to occupy a volume larger than what it would occupy if it were ideal.

18
Q

How does strength of IMF affect deviation of pV/RT?

A

Atoms/compounds with stronger IMF deviate more than those with weaker IMF.

19
Q

How does size of atoms/compounds affect deviation of pV/RT?

A

The larger the size of the atom/compound, the more easily it is able to be polarised, the stronger its IMF interactions, the more it deviates from ideality.

20
Q

What is Dalton’s Law of Partial Pressures?

A

The total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases in the mixture.

21
Q

What is the mole fraction of a component A?

A

The ratio of the number of moles of the gas A to the total number of moles of all gaseous components present in the mixture.
x = number of moles of component A/total number of moles of all components in the mixture = na/ntotal

22
Q

What is the partial pressure of gas A?

A

The product of the mole fraction of A in the mixture and the total pressure of the mixture.
PA = (xA)(Ptotal)

23
Q

What is saturated vapour pressure?

A

The vapour pressure exerted by a fixed number of gaseous particles in a dynamic equilibrium at a particular temperature.

24
Q

How does the strength of the IMF of a liquid affect its volatility, saturated vapour pressure and boiling point?

A

The stronger the IMF, the lower the volatility and saturated vapour pressure, the higher its boiling point.

Chemistry (8 decks)

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