Upload
milton-junior-wheeler
View
216
Download
0
Tags:
Embed Size (px)
Citation preview
Ideal Gas Law
The equality for the four variables involved in Boyle’s Law, Charles’ Law, Gay-Lussac’s Law and Avogadro’s law can be written
PV = nRT
R = ideal gas constant
Ideal Gases
Behave as described by the ideal gas equation; no real gas is actually ideal
Within a few %, ideal gas equation describes most real gases at room temperature and pressures of 1 atm or less
In real gases, particles attract each other reducing the pressure
Real gases behave more like ideal gases as pressure approaches zero.
PV = nRT
R is known as the universal gas constant
Using STP conditions P V
R = PV = (1.00 atm)(22.4 L) nT (1mol) (273K)
n T
= 0.08205 L-atm
mol-K
Understanding the Ideal Gas Law
What is the value of R when the STP value for P is 760 mmHg?
Solution
What is the value of R when the STP value for P is 760 mmHg?
R = PV = (760 mm Hg) (22.4 L)
nT (1mol) (273K)
= 62.4 L-mm Hg mol-K
Understanding Gas Laws
Dinitrogen oxide (N2O), laughing gas, is used by dentists as an anesthetic. If 2.86 mol of gas occupies a 20.0 L tank at 23°C, what is the pressure (mmHg) in the tank in the dentist office?
Solution
Set up data for 3 of the 4 gas variables
Adjust to match the units of R
V = 20.0 L 20.0 L
T = 23°C + 273 296 K
n = 2.86 mol 2.86 mol
P = ? ?
Rearrange ideal gas law for unknown P
P = nRT
V
Substitute values of n, R, T and V and solve for P
P = (2.86 mol)(62.4L-mmHg)(296 K)
(20.0 L) (K-mol)
= 2.64 x 103 mm Hg
Check your understanding
A 5.0 L cylinder contains oxygen gas at 20.0°C and 735 mm Hg. How many grams of oxygen are in the cylinder?
Solution
Solve ideal gas equation for n (moles)n = PV
RT
= (735 mmHg)(5.0 L)(mol K) (62.4 mmHg L)(293 K)
= 0. 20 mol O2 x 32.0 g O2 = 6.4 g O2
1 mol O2
Molar Mass of a gas
What is the molar mass of a gas if 0.250 g of the gas occupy 215 mL at 0.813 atm and 30.0°C?
n = PV = (0.813 atm) (0.215 L) = 0.00703 mol
RT (0.0821 L-atm/molK) (303K)
Molar mass = g = 0.250 g = 35.6 g/mol
mol 0.00703 mol
Density of a Gas
Calculate the density in g/L of O2 gas at STP. From STP, we know the P and T.
P = 1.00 atm T = 273 K
Rearrange the ideal gas equation for moles/L
PV = nRT PV = nRT P = n
RTV RTV RT V
Substitute
(1.00 atm ) mol-K = 0.0446 mol O2/L
(0.0821 L-atm) (273 K)
Change moles/L to g/L
0.0446 mol O2 x 32.0 g O2 = 1.43 g/L
1 L 1 mol O2
Therefore the density of O2 gas at STP is
1.43 grams per liter
Formulas of Gases
A gas has a % composition by mass of 85.7% carbon and 14.3% hydrogen. At STP the density of the gas is 2.50 g/L. What is the molecular formula of the gas?
Formulas of Gases
Calculate Empirical formula
85.7 g C x 1 mol C = 7.14 mol C/7.14 = 1 C 12.0 g C
14.3 g H x 1 mol H = 14.3 mol H/ 7.14 = 2 H 1.0 g H
Empirical formula = CH2
EF mass = 12.0 + 2(1.0) = 14.0 g/EF
Using STP and density ( 1 L = 2.50 g)
2.50 g x 22.4 L = 56.0 g/mol
1 L 1 mol
n = EF/ mol = 56.0 g/mol = 4
14.0 g/EF
molecular formula
CH2 x 4 = C4H8
Gases in Chemical Equations
On December 1, 1783, Charles used 1.00 x 103 lb of iron filings to make the first ascent in a balloon filled with hydrogen
Fe(s) + H2SO4(aq) FeSO4(aq) + H2(g)
At STP, how many liters of hydrogen
gas were generated?
Solution
lb Fe g Fe mol Fe mol H2 L H2
1.00 x 103 lb x 453.6 g x 1 mol Fe x 1 mol H2
1 lb 55.9 g 1 mol Fe
x 22.4 L H2 = 1.82 x 105 L H2
1 mol H2
Charles generated 182,000 L of hydrogen to fill his air balloon.
Check your understanding
How many L of O2 are need to react 28.0 g NH3 at 24°C and 0.950 atm?
4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)
Solution
Find mole of O2
28.0 g NH3 x 1 mol NH3 x 5 mol O2
17.0 g NH3 4 mol NH3
= 2.06 mol O2
V = nRT = (2.06 mol)(0.0821)(297K) = 52.9 L
P 0.950 atm
Summary of Conversions with Gases
Volume A Volume B
Grams A Moles A Moles B Grams B
Atoms or Atoms or
molecules A molecules B
Daltons’ Law of Partial Pressures
The % of gases in air Partial pressure (STP)
78.08% N2 593.4 mmHg
20.95% O2 159.2 mmHg
0.94% Ar 7.1 mmHg
0.03% CO2 0.2 mmHg
PAIR = PN + PO + PAr + PCO = 760 mmHg 2 2 2
Total Pressure 760 mm Hg
Check your understanding
A.If the atmospheric pressure today is 745 mm Hg, what is the partial pressure (mm Hg) of O2 in the air?
1) 35.6 2) 156 3) 760
B. At an atmospheric pressure of 714, what is the partial pressure (mm Hg) N2 in the air?
1) 557 2) 9.14 3) 0.109
Solution
A.If the atmospheric pressure today is 745 mm Hg, what is the partial pressure (mm Hg) of O2 in the air?
2) 156
B. At an atmospheric pressure of 714, what is the partial pressure (mm Hg) N2 in the air?
1) 557
Partial Pressure
Partial Pressure
Pressure each gas in a mixture would exert if it were the only gas in the container
Dalton's Law of Partial PressuresThe total pressure exerted by a gas mixture is the sum of the partial pressures of the gases in that mixture.
PT = P1 + P2 + P3 + .....
Partial Pressures
The total pressure of a gas mixture depends
on the total number of gas particles, not on
the types of particles.
STP
P = 1.00 atm P = 1.00 atm
1.0 mol He0.50 mol O2
+ 0.20 mol He+ 0.30 mol N2
Check your understanding
A 5.00 L scuba tank contains 1.05 mole of O2 and 0.418 mole He at 25°C. What is the partial pressure of each gas, and what is the total pressure in the tank?
Solution
P = nRT PT = PO + PHe
V 2
PT = 1.47 mol x 0.0821 L-atm x 298 K
5.00 L (K mol)
= 7.19 atm