Chapter 14
#59 Parts of the kinetic molecular theory
-All matter is made up of ____ _________
- All particles are in constant ______
-Collisions between these particles are _______________
# 60 Ideal Gas
-It’s a gas that when kept at a constant temperature, would obey the ___ ____exactly. No known gas in
an ideal gas
# 61 Elastic collision - An encounter between two particles, in which
______________________________.
#62 Effusion - the movement of a gas through a ___________________ into another gaseous region.
#63 Boyles Law (P1V1=P2V2)
- Example: A balloon with a volume of 2.0L is filled with a gas at 3atm. If the pressure was reduced to
0.5atm without a temperature change, what would be the volume of the balloon?
#64 Charles Law (V1T1=V2T2)
-A certain amount of gas occupies a volume of 60 L at 300 K. find the temperature if the amount of gas
at 100 L.
#65 Gay-Lussac Law(P1/T1=P2/T2)
-A 20 L cylinder containing 6atm of gas at 27 C+273K. What would the pressure of the gas if it was
heated to 77 C+273K?
# 66 Combined Gas Law
-Given : V1 = 30 L
V2 = ???
T1 = 313 K
T2 = 273 K
P1 = 153 kPa
P2 = 101.3 kPa
Use = P1*V1/T1 = P2*V2 /T2
Solve =
#67 If the Temperature is Constant, As the Pressure Increases the Volume _______
If the Pressure is Constant, As the Temperature Increases the Volume _______
If the Volume is Constant, As the Temperature Increases the Pressure _______
#68-69 Absolute Zero is the base for the Kelvin scale.
Absolute Zero = ___________________________________
STP = _________________________________
(101.3kPa = 101300 Pa = 1atm)
101.3 kPa = 101,300 Pa = 1 atm
#70, 71, 72
Dalton’s Law: In a Mixture of Gases, the total Pressure is the sum of the partial pressures of the separate
gases. (Ptotal=________________________)
Ptotal = 101.3 kPa
PN2 = 79.10 / PCO2 = 0.040 / Pothers = 0.94
PN2 + PCO2 + Pothers + PO2 = 101.3
Find PO2
7 Gas Laws :
-Boyle’s Law (P1V1 = P2V2)
-Charles’ Law (V1/T1 = V2/T2)
- Gay Lussac’s Law (P1/T1 = P2/T2)
-Combined Gas Law (P1V1/T1 = P2V2/T2)
-Ideal Gas Law (PV = nRT)
- Dalton’s Law of Partial Pressure (Ptotal = P1 + P2 + P3 +…)
- Graham’s Law (Rate A/RateB = √Molar MassB / √ Molar Mass)
# 73 A gas as a pressure of 1.26 atm and occupies a volume of 7.4 L. If the gas is compressed to a volume
of 2.93L, what will the pressure be assuming the temperature is constant?
Given = P1 = 1.26atm
V2 = 67.4 L
P2 = ?
V2 = 2.93 L
Find : P2
Use : Boyle’s Law
Solve =
#74 A helium gas filled balloon has a volume of 2.75L at 20°C. The volume of the balloon decreases to
2.46L after it is placed outside on a cold day, what is the outside temperature?
Given : V1 = 2.75L
V2 = 2.46L
T1 = 20°C = 293 K T2 = ?
Find = T2
Use : Charles Law
Solve =
#75 A sample of helium gas has a pressure of 1.20 atm 22°C. At what celsius temperature will the helium
reach a pressure of a 2.00 atm? Given = P1 = 1.20 atm
P2 = 2 atm
T1 = 22°C = 295K
T2 = ?
Find = T2
Use = Gay Lussac’s Law
Solve =
#76 A 700 mL gas sample at STP is compressed to a volume of 200 mL and the temperature is increased
to 30°C. What is the new pressure of the gas in Pa?
Given = P1 = 101.300 Pa
P2 = ?
V1 = 700 mL
V2 = 200mL
T1 = 273 K
T2 = 303 K
Find = P2
Use = Combined Gas Law
Solve =
#77 A Helium filled balloon contains 0.16 mol He at 101kPa and a temperature of 23°C. What is the
volume of the gas in the balloon?
Given = P = 101kPa
V=?
T = 296K
n = 0.16 mol
R = 8.314 L*kPa/mol*K
Find = V
Use = Ideal Gas Law
Solve =
#78 Dalton's Law of Partial Pressure: The total pressure of a mixture of gasses is equal to the sum of the
partial pressure of the component gases. (Ptotal = P1 + P2 + P3 +…)
Ideal Gas Law : The mathematical relationship between pressure, volume, temperature, and the number
of moles of a gas. (PV = nRT)
Graham's Law of Effusion = The rates of effusion (R or V) of gases (at the same Temperature and
Pressure) are inversely proportional to the square root of their molar masses (Rate A/RateB = √Molar
MassB / √ Molar Mass)
#79 If the partial pressure of a Carbon dioxide, helium, and oxygen is 100 kPa, 80 kPa and 40 kPa
respectively, what is their total pressure?
Given = Pcarbondioxide = 100 kPa
Phelium = 80 kPa
Poxygen = 40 kPa
Find = Ptotal
Use = Dalton’s Law of Partial Pressure
Solve =
#80 Compare the rate of effusion of nitrogen and oxygen
Given = Molar mass of N2 = 28.0 g/mol
Molar mass of O2 = 32.00 g/mol
Use = Graham’s Law (Rate A/RateB = √Molar MassB / √ Molar Mass A)
Solve =