Chapter 11
Pages 361-385

Pressure (P) = Force/Area
◦ Units for P
 1 atm = 101.325 kPa = 760 mmHg = 760 torr = 14.7 psi
◦ Units for F
 Newton
◦ Units for A
 m2

Dalton’s Law of Partial Pressures
◦ Add partial pressures of all gases in mixture to find
total pressure

Demonstration (calculating your pressure)
practice conversions p.365

11.1 section review (#2-4, 6)
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
P.369-370
◦ K-M theory: explain the relationship between
pressure and volume
 As volume decreases, molecules collide more often
with the walls of their container, which increases
pressure. Pressure and volume are inversely related.
◦ Definition
◦ Equation (PV = PV)

Practice p.370

P.371-372
◦ K-M theory: explain the relationship between
volume and temperature
◦
◦
◦
◦

 As temperature increases, the number of collisions of
particles increase. If pressure is constant, volume
increases. Volume and temperature are directly
related.
Temperatures must be in Kelvin (oC + 273.15)
Absolute zero
Definition
Equation (V1 / T1 = V2 / T2)
Practice p.372

P.373-374
◦ K-M theory: explain the relationship between
pressure and temperature
 When temperature increases, the number of collisions
of particles increases, and pressure increases if volume
is constant. Pressure and temperature are directly
related.
◦ Definition
◦ Equation (P1 / T1 = P2 / T2 )

Practice p.374

P.374-375
◦ Definition
◦ Equation (PV / T = PV / T)

Practice p.375

Due today: 11.2 section review (all)




Define
Equation
Ideal gas constant: R = .0821 L·atm / mol·K
or 8.31 L·kPa/mol·K
Ideal gas law units:
◦
◦
◦
◦

V in liters
P in atm or kPa (changes value of R)
n in mol
T in K
Practice p.385

1 mole of gas = volume of ______ L
◦ Practice p.381

Remembering stoichiometry
◦ Write out the chemical equation
◦ Balance the equation
◦ Use molar ratios to convert from given to desired
answer
◦ Practice p.382
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
Practice p.385
Section review (#2, 3, 5-7)