Gas Laws Flashcards
Gas Particle Information
1) No volume compared to volume that the gas occupies - volume created by the motion of gas molecules.
2) Motion is constant and random in direction and speed.
3) All collisions between molecules are perfectly elastic (no loss of motion to other forms of energy).
Gas Laws
Mathematical relationships that describe properties of gases. (Each law can only be explained by the use of atoms - Kinetic Theory of Gases)
What is Pressure?
Number of collisions per surface area of container. (P = force/area)
Standard Pressures
1 ATM
760 mmHg
29.92 inHg
101.3 kPa
Boyle’s Law
For a fixed mass of gas at constant temperature, the pressure and volume of the gas varies indirectly.
P1V1 = P2V2
Charles’ Law
For a fixed mass of gas at constant pressure, the temperature and volume of a gas vary directly.
V1/T1 = V2/T2
Absolute Zero
0K
- 273*C
- 459*F
Where volume is zero and motion is zero.
Amanton Guy-Lussac’s Law
For a fixed mass of gas at constant volume, the Kelvin temperature and pressure vary directly.
P1/T1 = P2/V2
Maldenburg Spheres
When a vacuum is created inside of an object, the collisions outside of the object are much stronger than the inside. When the vacuum is broken, the collisions reach the same number and have equal strength.
The Combined Gas Law
P1V1/T1 = P2V2/T2
Dalton’s Gas Law
The total pressure for a mixture of gases is the sum of the individual pressures at the same conditions (volume and temperature).
Sum Indv. P = Total P
Calculating Dry Gas from Wet Gas
P ATM Outside = P Dry + P Vapor
Bromthymol Blue Indications
Green = Neutral Blue = Base/Alkaline Yellow = Acid/Acidic
Ideal Gas Law
PV = nRT
Universal Gas Constant (R)
- 21x10^-2 ATM•l/mol•k
- 31 kPa•l/mol•k
- 4 mmHg•l/mol•k
