Gaseous State Flashcards
1
Q
What is an ideal gas(important)
A
- volume of gas molecules is negligible compared to the volume of the container
- forces of attraction between the gas molecules as well as between gas molecules and the walls of the container are negligible
- all molecular collisions are perfectly elastic. No loss of kinetic energy during collision
2
Q
What is an ideal gas
A
- gases consist of rigid spherical molecules that are in continuous and random motion
- average kinetic energy of molecule is proportional to the absolute temperature
3
Q
Boyle’s Law: pressure-volume relationship
A
- volume of a fixed amount of gas is inversely proportional to its pressure under constant temperature
4
Q
Charles’s Law: temperature-volume relationship
A
- volume of a fixed amount of gas maintained at constant pressure is directly proportional to its absolute temperature
5
Q
Gay Lussac’s Law: temperature-pressure relationship
A
- pressure of a fixed amount of gas maintained at constant volume is directly proportional to its absolute temperature
6
Q
Avogadro’s Law: quantity-volume relationship
A
- at constant temperature and pressure the volume of a gas is directly proportional to the number of moles of the gas
7
Q
Ideal gas equation
A
- pv=nRT
- r = 8.31
8
Q
What is partial pressure
A
- partial pressure of a gas is equal to the pressure that the gas would exert as if it alone occupied the container
9
Q
Dalton’s Law of Partial Pressure
A
- states that in a mixture of gases which does not react chemically, the total pressure is the sum of the partial pressures of all the constituent gases at the same temperature
10
Q
Conditions to approach ideal behaviour
A
- Low pressure: when pressure is low, the gas molecules are far apart. The volume of gas molecules therefore becomes insignificant compared to the volume of the container and intermolecular forces of attraction are negligible
- High temperature: when temperature is high the gas molecules move faster and the intermolecular forces of attraction becomes negligible
11
Q
Why are there deviations from Ideal behaviour
A
- the strength of intermolecular forces of attraction and molecular volume causes different gases to deviate differently from ideality
