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# Ideal Gas Equation

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### Transcript

• 1. Boyle’s law: V a (at constant n and T)
Va
nT
nT
nT
P
P
P
V = constant x = R
1
P
Ideal Gas Equation
Charles’ law: VaT(at constant n and P)
Avogadro’s law: V a n(at constant P and T)
R is the gas constant
PV = nRT
• 2. The Universal Gas Constant
The conditions 0 0C and 1 atm are called standard temperature and pressure (STP).
Experiments show that at STP, 1 mole of an ideal gas occupies 22.414 L.
PV = nRT
R = PV/nT
At STP R = (1 atm)(22.414L)
(1 mol)(273.15 K)
R = 0.082057 L•atm mol • K
• 3. 1 mol HCl
V =
n = 49.8 g x
= 1.37 mol
36.45 g HCl
1.37 mol x 0.0821 x 273.15 K
V =
1 atm
nRT
L•atm
P
mol•K
What is the volume (in liters) occupied by 49.8 g of HCl at STP?
T = 0 0C = 273.15 K
P = 1 atm
PV = nRT
V = 30.6 L
• 4. m
V
PM
=
RT
dRT
P
Density (d) Calculations
m is the mass of the gas in g
d =
M is the molar mass of the gas
Molar Mass (M ) of a Gaseous Substance
d is the density of the gas in g/L
M =
• 5. What is the volume of CO2 produced at 370 C and 1.00 atm when 5.60 g of glucose are used up in the reaction:
C6H12O6 (s) + 6O2 (g) 6CO2 (g) + 6H2O (l)
6 mol CO2
g C6H12O6 mol C6H12O6 mol CO2V CO2
x
1 mol C6H12O6
1 mol C6H12O6
x
180 g C6H12O6
L•atm
mol•K
nRT
0.187 mol x 0.0821 x 310.15 K
=
P
1.00 atm
Gas Stoichiometry
5.60 g C6H12O6
= 0.187 mol CO2
V =
= 4.76 L