Gaseous State Flashcards
What does the Avogadro’s Law state?
The volume, V, of a gas is directly proportional to the amount of gas particles(in mol) at constant temperature and pressure
V1/N1 = V2/N2
What is the standard temperature and pressure and the respective molar volume?
- 0 degree celsius (273K)
- 1 bar (10^5 Pa)
- Vm=22.7dm3
What is the room temperature and pressure and its respective molar volume?
- 20 degree celsius (293K)
- 1 atm (101325 Pa)
- Vm=24dm3
What does the Boyle’s Law state?
The volume of a fixed mass of a gas is inversely proportional to its pressure at a constant temperature
p1 V1=p2 V2
What does the Charle’s Law state?
It states that the volume of a fixed mass of a gas is directly proportional to its absoulte temperature (in K) at a constant pressure.
V1/T1=V2/T2
What does the Gay-Lussac’s Law states?
The pressure of a fixed mass of gas is directly proportional to its absolute temperature (in K) at a constant volume.
p1/T1=p2/T2
What is the value of molar gas constant?
8.31(J K-1 mol-1)
What does the Dalton’s Law state?
It states that the total pressure of a mixture of gases that do not react chemically with one another is the sum of the partial pressure of the constituent gases.
What are the assumptions of kinetic theory of gases?
1.There are no intermolecular forces of attraction between particles of an ideal gas.
2. The volume of the ideal gas particles is negligible as compared to the volume of the container.
3. Collisions between particles of an ideal gas are perfectly elastic.
- Gas particles(atoms, molecules) are in rapid, continuous and random motion.
- The average kinetic energy of the particles is proportional to its absolute temperature measured in Kelvin
How does pressure affect the deviation of gases from ideal behaviour?
Gas deviates from ideal behaviour more at a higher pressure as
- volume of containter decreases and the particles are packed closer together
- so the volume of the particles become significant compared to the volume of the containter.
How does temperature affect the deviation gases from ideal behaviour?
Gas deviates from ideal behaviour more at lower temperature as
- particles have less kinetic energy and will move slower, hence collide with one another with less force.
- This makes IMFOA more significant compared to the forces of intermolecular collisions.
Why does real gases behave most ideally at low pressure and high temperatures?
At low pressure, the particles are far apart from each other and volume of container increases. Thus, the volume of the gases becomes negligible to the volume of the container.
At high temperatures, the particles have a higher average kinetic energy and move faster and overcome the intermolecular forces of attraction. Thus, the IMFOA of gases becomes negligible compared to forces of intermolecular collisions.
