5.1 Pressure . Pressure a. Devices used to measure pressure 1. Barometer: measures atmospheric pressure *Atmospheric pressure results from the mass of air being pulled toward the center of the earth by gravity.
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a. Devices used to measure pressure
1. Barometer: measures atmospheric pressure
*Atmospheric pressure results from the mass of air being pulled toward the center of the earth by gravity.
2. Manometer: measures the pressure of a gas in a container
b. Units of Pressure
1. mmHg = Torr (invented the first barometer)
2. 1 atm = 760 mmHg = 760 torr = 1.013 x 105 Pa
3. Pressure = force/ area
*pressure, temp, vol, amount
A. Boyle’s Law: volume and pressure are inversely related at constant temp
PV = k
P1V1 = P2V2
B. Charles’ Law: Kelvin temperature and volume vary directly with each other at constant temperature.
*if you graph a line of V vs. T all lines extrapolate to zero volume at 0K.
*V1/ T1 = V2/ T2
C. Avogadro’s Law: for a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas present
* V1/ n1 = V2/ n2
A. PV = nRT, R = 0.08206 Latm/ Kmol
B. Gas laws describe ideal gases, not real gases
C. Real gas behavior approaches ideal at high temps and low pressures
A. The moalr volume of a gas at STP is 22.4 L ideally
B. STP 0oC, 1atm (273 K, 1.013 x 105Pa)
CH4(g) + 2O2(g) CO2(g) + 2H2O (g)
CO2(g) __L @ 125oC 2.50 atm
C. n = grams of gas/ molar mass
D = m/v
P = dRT/ molar mass
A. Ptotal = P1 + P2 + P3 + …
B. Calculate the partial pressure using the ideal gas law
Ptotal = (n1 + n2…) RT/V
C. Total pressure depends on the total number of moles of gas, not the identity of the particles
D. Mole fraction is the ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture (x = chi)
x = n2/ ntotal = P2/ Ptotal
n = PV/RT if V, R, T are constant then n = P
*the partial pressure of a particular component of a gaseous mixture is the mole fraction of that component times the total pressure
-based on observations used to explain and predict the behavior of ideal gases
A. Volume of particles can be assumed to be negligible
B. Particles are in constant motion, pressure is created by the collision of particles with the walls of the container
C. The particles are assumed to exert no forces on each other
D. The average KE of a collection of gas particles is assumed to be directly proportional to the Kelvin temp. of the gas.
A. Graham’s Law: the rate of effusion of a gas is inversely proportional to the square root of the mass of the particles of gas
B. Diffusion: mixing of gases due to random motion of particles
A. No gas exactly follows ideal gas behavior (close under high temp, and low pressure)
B. Van der Waal’s equation: describes the behavior of a real gas by correcting for the actual volume of gas particles and forces between gas particles
[Pobs + a(n/v)2] x (V – nb) = nRT
Pobs = observed pressure
a(n/v)2 = pressure correction
V = volume of container
V – nb = volume correction
*a and b are constants obtained from observation of real gases
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