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0.0821 (L*atm)/(mol*K)
62.3 (L*mmHg)/(mol*K)
Ptotal = P1 + P2 +…Pn
were P1 is the partial pressure of gas one, P2 is the partial pressure of gas two (and so on)
Pgas = Ptot - PH2O
where PH2O is the vaper pressure of water
P1 = X1 * Ptot
where X1 is the mole fractio
Etrans = 1/2 * m * u^2 = C * T
m1u1^2 = m2u2^2
rate2/rate1 = (M1/M2)^(1/2) = time1/time2
u = (3RT/M)^(1/2) where R = 8.31 (g*m^2)/(s^2*mol*K)
real gases deviate from ideal gases
gas molecules attract each other
gas molecules occupy a finite volume
they deviate most at high pressures and low temps (smaller mean free path) and least at low pressures and high temperatures (bigger mean free path)
deviation is so small it’s negligible
explains the effects of temperature and pressure on matter
all matter is composed of small particle
these particles are in constant motion
collisions between particles are perfectly elastic (no change in total kinetic energy of the system)
created by the force and the number of gas molecule collisions on a container wall
pascal is the SI unit of pressure (1 Pa = 1 N/m^2)
101.325 kPa = 1 atm = 760 mm Hg
nanometers and barometers are used to measure gas pressure using column of mercury
nanometers - open and closed arm
