Chapter 05: Gases Flashcards
Pressure
The force exerted per unit area by gas molecules as they strike the surfaces around them
Pressure = force/area = F/A
Pressure units & conversion factors
760 mmHg = 760 torr = 1 atm = 101,325 Pa
Elements that exist as gases at 25°C and 1 atm
1A: H
5A: N
6A: O
7A: F, Cl
8A: (all)
Force (formula)
mass × acceleration
SI units of force and pressure
Force: 1 newton (N)
Pressure: 1 pascal (Pa)
Newton
1 newton = 1 kg×m/s2
Pascal
1 pascal = 1N/m2 = 1 kg/(m×s2)
Barometer
Atmospheric pressure measurment tool
Inverted tube of Hg over open dish of Hg;
height of Hg in mm is equal to atmospheric pressure
Manometer
Instrument used to measure pressure of gas trapped in container
Gas pressure is determined by difference in liquid levels in U-shaped tube
(Pressure is high if it pushes down on liquid;
low if it cannot push down on liquid)
Simple Gas Laws: Four* basic properties of a gas
P, pressure
V, volume
T, temperature (Kelvin)
t, temperature (°C)
n, amount in moles
Boyle’s law
Inverse relationship between volume and pressure
*n is constant
*T is constant
P1V1 = P2V2
Charles’ law
Direct relationship between volume and temperature (Kelvin).
*P is constant
*n is constant
V1 = V2
T1 T2
Avogadro’s law
Direct relationship between volume and quantity (number of moles)
*P is constant
*T is constant
V1 = V2
n n
Ideal Gas Law
How a hypothetical gas behaves
PV = nRT
Where R is the ideal gas constant
R, ideal gas constant
R = 0.08206 L atm/mol K
Molar volume
The volume occupied by one mole of a substance
Ideal gas molar volume
22.414 L at STP of an ideal gas