The Gaseous State 🌪

0.0(0)
Studied by 0 people
call kaiCall Kai
Locked
learnLearn
examPractice Test
spaced repetitionSpaced Repetition
heart puzzleMatch
flashcardsFlashcards
GameKnowt Play
Card Sorting

1/6

encourage image

There's no tags or description

Looks like no tags are added yet.

Last updated 1:38 AM on 9/13/26
Name
Mastery
Learn
Test
Matching
Spaced
Call with Kai
Chat

No analytics yet

Send a link to your students to track their progress

7 Terms

1
New cards

State the basic assumptions of the kinetic theory as applied to an ideal gas

  1. The gas consists of particles of negligible volume compared to the volume of the container it occupies.

  2. The gas particles exert no attractive forces on each other.

  3. The collisions between gas particles are perfectly elastic and no kinetic energy is lost upon collision.


2
New cards

Explain why real gases tend to exhibit negative deviation when the temperature is low

  1. At low temperature, kinetic energy of gas particles is low and they move slower.

  2. Intermolecular forces of attraction between gas particles are significant.

  3. Gas particles collide with the container walls with lower frequency and with less force.

  4. Therefore, preal< pideal, prealV/RT< pidealV/RT= 1. The gas exhibits negative deviation.


3
New cards

State and explain the degree of negative deviation between NH3, N2 and H2

  1. Degree of negative deviation shown by NH3> N2> H2.

  2. Strength of hydrogen bonds between NH3 molecules> strength of instantaneous dipole induced dipole attractions between N2 molecules and H2 molecules.

  3. Size of electron cloud N2> H2. Extent of polarisation of N2 electron cloud> H2 electron cloud. Strength and extensiveness of instantaneous dipole induced dipole attractions between N2 molecules> H2 molecules.

  4. Collision frequency and collision force with container walls by NH3 molecules< N2 molecules< H2 molecules.

  5. Therefore, preal(NH3)< preal(N2)< preal(H2).


<ol><li><p>Degree of negative deviation shown by NH3&gt; N2&gt; H2.</p></li><li><p>Strength of hydrogen bonds between NH3 molecules&gt; strength of instantaneous dipole induced dipole attractions between N2 molecules and H2 molecules.</p></li><li><p>Size of electron cloud N2&gt; H2. Extent of polarisation of N2 electron cloud&gt; H2 electron cloud. Strength and extensiveness of instantaneous dipole induced dipole attractions between N2 molecules&gt; H2 molecules.</p></li><li><p>Collision frequency and collision force with container walls by NH3 molecules&lt; N2 molecules&lt; H2 molecules.</p></li><li><p>Therefore, preal(NH3)&lt; preal(N2)&lt; preal(H2).</p></li></ol><p></p>
4
New cards

Explain why real gases tend to exhibit positive deviation when the pressure is high

  1. At high pressures, the gas particles are closer together.

  2. Volume of the gas particles is significant compared to the total volume of the gas.

  3. Therefore, V real> Videal, pVreal/RT> pVideal/RT= 1. The gas exhibits positive deviation.


5
New cards

State and explain the degree of positive deviation between NH3, N2 and H2

  1. Degree of positive deviation shown by NH3> N2> H2.

  2. Molecular size of NH3> N2> H2.

  3. Volume of NH3 molecules is most significant compared to the total volume of the gas.

  4. Therefore, Vreal(NH3)> Vreal(N2)> Vreal(H2).


6
New cards

State and explain the conditions necessary for real gases to approach ideal gas behaviour

  1. At low pressure, the gas particles are far apart.

  2. The volume of the gas particles is insignificant compared to the total volume of the gas.

  3. At high temperature, the gas particles have sufficient kinetic energy to overcome the intermolecular forces of attraction which can be considered insignificant.


7
New cards

State Dalton’s Law of Partial Pressures

  1. The total pressure exerted by a mixture of gases which do not react is equal to the sum of the partial pressures of the constituent gases at the same temperature.