Transcript You are given an aqueous solution that contains a Co 2

11.1
All of the following are postulates of the kinetic
molecular theory of gases EXCEPT:
1. The volume occupied by a gas is mostly empty space.
2. The average kinetic energy of the gas particles is
proportional to the temperature in Celsius.
3. The attraction/repulsion between gas molecules is very
weak or negligible.
4. Gas molecules or atoms move in a straight line between
collisions.
5. All of the above are correct postulates.
Tro IC3
11.1
All of the following are postulates of the kinetic
molecular theory of gases EXCEPT:
1. The volume occupied by a gas is mostly empty space.
2. The average kinetic energy of the gas particles is
proportional to the temperature in Celsius.
3. The attraction/repulsion between gas molecules is very
weak or negligible.
4. Gas molecules or atoms move in a straight line between
collisions.
5. All of the above are correct postulates.
Tro IC3
11.2
Convert 580 mm Hg to atm:
1.
2.
3.
4.
5.
Tro IC3
0.763
atm
1.00
atm
5.80
atm
580
atm
4.41 x 105 atm
11.2
Convert 580 mm Hg to atm:
1.
2.
3.
4.
5.
Tro IC3
0.763
atm
1.00
atm
5.80
atm
580
atm
4.41 x 105 atm
11.3
Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi
and 1 atm = 101325 Pa.)
1.
2.
3.
4.
5.
Tro IC3
2.41
kPa
2.45 x 102 kPa
5.29 x 102 kPa
2.45 x 105 kPa
5.29 x 105 kPa
11.3
Convert 35.5 psi to kPa. (Note: 1 atm = 14.7 psi
and 1 atm = 101325 Pa.)
1.
2.
3.
4.
5.
Tro IC3
2.41
kPa
2.45 x 102 kPa
5.29 x 102 kPa
2.45 x 105 kPa
5.29 x 105 kPa
11.4
A gas has a volume of 1.0 L at 1 atm. By what
factor must the pressure change in order to halve
the volume of the gas? (Assume the temperature is
constant.)
1.
2.
3.
4.
5.
Tro IC3
x1
x2
x4
x 1/2
x 1/4
11.4
A gas has a volume of 1.0 L at 1 atm. By what
factor must the pressure change in order to halve
the volume of the gas? (Assume the temperature is
constant.)
1.
2.
3.
4.
5.
Tro IC3
x1
x2
x4
x 1/2
x 1/4
11.5
A bottle with 500 mL of a liquid is sealed on top of
Mt. Everest (P = 230 torr). What is the volume of
the liquid when the bottle is moved to sea level?
(Assume the temperature is kept constant.)
1.
2.
3.
4.
5.
Tro IC3
651
mL
1.65 x 103 mL
0.151
mL
151
mL
500.
mL
11.5
A bottle with 500 mL of a liquid is sealed on top of
Mt. Everest (P = 230 torr). What is the volume of
the liquid when the bottle is moved to sea level?
(Assume the temperature is kept constant.)
1.
2.
3.
4.
5.
Tro IC3
651
mL
1.65 x 103 mL
0.151
mL
151
mL
500
mL
11.6
What is absolute zero?
1.
2.
3.
4.
5.
Tro IC3
-273°F
The freezing point of hydrogen
The x-intercept of a straight-line graph of V versus 1/P
The x-intercept of a straight-line graph of V versus T
The temperature of deep outer space
11.6
What is absolute zero?
1.
2.
3.
4.
5.
Tro IC3
-273°F
The freezing point of hydrogen
The x-intercept of a straight-line graph of V versus 1/P
The x-intercept of a straight-line graph of V versus T
The temperature of deep outer space
11.7
A flexible container contains 1.50 L of gas at 25 °C.
What is the new volume when the container is heated
to 100 °C? (Assume the pressure is constant.)
1.
2.
3.
4.
5.
Tro IC3
0.375 L
0.959 L
1.20 L
0.833 L
1.88 L
11.7
A flexible container contains 1.50 L of gas at 25 °C.
What is the new volume when the container is heated
to 100 °C? (Assume the pressure is constant.)
1.
2.
3.
4.
5.
Tro IC3
0.375 L
0.959 L
1.20 L
0.833 L
1.88 L
11.8
A bottle with 500 mL of a liquid is sealed on top of
Mt. Everest (230 torr) at a temperature of -20 °C.
What is the approximate volume of the liquid when
the bottle is moved to sea level at a temperature of
30.0 °C?
1.
2.
3.
4.
5.
Tro IC3
100 mL
126 mL
180 mL
500 mL
680 mL
11.8
A bottle with 500 mL of a liquid is sealed on top of
Mt. Everest (230 torr) at a temperature of -20 °C.
What is the approximate volume of the liquid when
the bottle is moved to sea level at a temperature of
30.0 °C?
1.
2.
3.
4.
5.
Tro IC3
100 mL
126 mL
180 mL
500 mL
680 mL
11.9
What law is derived from the combined gas law
under constant temperature and moles?
1.
2.
3.
4.
5.
Tro IC3
Avogadro’s
Charles’s
Dalton’s
Gay-Lussac’s
Boyle’s
11.9
What law is derived from the combined gas law
under constant temperature and moles?
1.
2.
3.
4.
5.
Tro IC3
Avogadro’s
Charles’s
Dalton’s
Gay-Lussac’s
Boyle’s
11.10
A container with 1.00 mol of gas is expanded from
5.00 L to 10.0 L by adding more gas. The
temperature and pressure are kept constant. How
many moles of gas are present after the expansion?
1.
2.
3.
4.
5.
Tro IC3
1.00 mol
2.00 mol
3.00 mol
5.00 mol
10.0 mol
11.10
A container with 1.00 mol of gas is expanded from
5.00 L to 10.0 L by adding more gas. The
temperature and pressure are kept constant. How
many moles of gas are present after the expansion?
1.
2.
3.
4.
5.
Tro IC3
1.00 mol
2.00 mol
3.00 mol
5.00 mol
10.0 mol
11.11
A set of car tires contain a volume of 45.5 L of air at
35.0 psi and 0 °C. When the car is driven, the
temperature of the tires increases to 40 °C. What is
the pressure (in psi) of each tire assuming constant
volume?
1.
2.
3.
4.
5.
Tro IC3
37.8 psi
35.0 psi
0
psi
40.1 psi
29.9 psi
11.11
A set of car tires contain a volume of 45.5 L of air at
35.0 psi and 0 °C. When the car is driven, the
temperature of the tires increases to 40 °C. What is
the pressure (in psi) of each tire assuming constant
volume?
1.
2.
3.
4.
5.
Tro IC3
37.8 psi
35.0 psi
0
psi
40.1 psi
29.9 psi
11.12
How many moles of an ideal gas are in a container
with a volume of 5.50 L at 580 mm Hg and 20 °C?
Note: R = 0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
1.32 mol
0.229 mol
0.174 mol
2.58 mol
5.73 mol
11.12
How many moles of an ideal gas are in a container
with a volume of 5.50 L at 580 mm Hg and 20 °C?
Note: R = 0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
1.32 mol
0.229 mol
0.174 mol
2.58 mol
5.73 mol
11.13
What is the volume occupied by 28.0 g of nitrogen
gas at 1.00 atm and 0 °C? Note: R = 0.0821
L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
0.0295 L
1.00 L
22.4 L
48.8 L
0.0446 L
11.13
What is the volume occupied by 28.0 g of nitrogen
gas at 1.00 atm and 0 °C? Note: R = 0.0821
L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
0.0295 L
1.00 L
22.4 L
48.8 L
0.0446 L
11.14
A 4.17-g sample of particular ideal diatomic gas at
38 °C has a volume of 1.50 L at 1.00 atm. Identify
the gas? Note: R = 0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
H2
N2
F2
O2
Cl2
11.14
A 4.17-g sample of particular ideal diatomic gas at
38 °C has a volume of 1.50 L at 1.00 atm. Identify
the gas? Note: R = 0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
H2
N2
F2
O2
Cl2
11.15
A real gas can approach ideal behavior:
1.
2.
3.
4.
5.
Tro IC3
When both the pressure and temperature are high
When the pressure is high and the temperature is low
When both the pressure and temperature are low
When the pressure is low and the temperature is high
Real gases have ideal behavior no matter what the
conditions are.
11.15
A real gas can approach ideal behavior:
1.
2.
3.
4.
5.
Tro IC3
When both the pressure and temperature are high
When the pressure is high and the temperature is low
When both the pressure and temperature are low
When the pressure is low and the temperature is high
Real gases have ideal behavior no matter what the
conditions are.
11.16
Calculate the molar mass of a gas that has a
density of 1.70 g/L at STP.
1.
2.
3.
4.
5.
Tro IC3
2.02 g/mol
4.00 g/mol
28.0 g/mol
32.0 g/mol
38.1 g/mol
11.16
Calculate the molar mass of a gas that has a
density of 1.70 g/L at STP.
1.
2.
3.
4.
5.
Tro IC3
2.02 g/mol
4.00 g/mol
28.0 g/mol
32.0 g/mol
38.1 g/mol
11.17
1.
2.
3.
4.
5.
Tro IC3
The partial pressures in a mixture of CO2, N2, and
O2 in a sample of gas are 50.0 atm, 495 atm, and
205 atm, respectively. Calculate the mole
percentage of each gas.
5.00%, 70.3%, 24.7%
6.67%, 66.0%, 27.3%
0.500%, 49.5%, 50.0%
10.0%, 50.0%, 40.0%
1.50%, 75.5%, 23.0%
11.17
1.
2.
3.
4.
5.
Tro IC3
The partial pressures in a mixture of CO2, N2, and
O2 in a sample of gas are 50.0 atm, 495 atm, and
205 atm, respectively. Calculate the mole
percentage of each gas.
5.00%, 70.3%, 24.7%
6.67%, 66.0%, 27.3%
0.500%, 49.5%, 50.0%
10.0%, 50.0%, 40.0%
1.50%, 75.5%, 23.0%
11.18
A sample of hydrogen gas is collected over water at
a pressure of 635 mm Hg at 10.0 °C. Calculate
partial pressure of the hydrogen. The vapor
pressure over water at 10.0 °C is 9.2 mm Hg.
1.
9 mm Hg
2. 69 mm Hg
3. 626 mm Hg
4. 635 mm Hg
5. 644 mm Hg
Tro IC3
11.18
A sample of hydrogen gas is collected over water at
a pressure of 635 mm Hg at 10.0 °C. Calculate
partial pressure of the hydrogen. The vapor
pressure over water at 10.0 °C is 9.2 mm Hg.
1.
9 mm Hg
2. 69 mm Hg
3. 626 mm Hg
4. 635 mm Hg
5. 644 mm Hg
Tro IC3
11.19
How many liters of dry oxygen gas are produced by
the complete electrolysis of 225 mL of water? The
oxygen gas is collected at 580 torr and 27 °C. The
density of water at 27 °C is 1.00 g/mL. Note: R =
0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
0.225 L
36.3 L
201
L
403
L
0.0239 L
11.19
How many liters of dry oxygen gas are produced by
the complete electrolysis of 225 mL of water? The
oxygen gas is collected at 580 torr and 27 °C. The
density of water at 27 °C is 1.00 g/mL. Note: R =
0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
0.225 L
36.3 L
201
L
403
L
0.0239 L
11.20
How many grams of water are produced from the
complete combustion of 15.8 L of propane (C3H8)
gas at STP?
1.
2.
3.
4.
5.
Tro IC3
0.705 g
2.82 g
12.7 g
38.1 g
50.8 g
11.20
How many grams of water are produced from the
complete combustion of 15.8 L of propane (C3H8)
gas at STP?
1.
2.
3.
4.
5.
Tro IC3
0.705 g
2.82 g
12.7 g
38.1 g
50.8 g
11.21
Which of the following samples occupy the largest
volume at STP? Note: R = 0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
1.00 mol O2
48.0 g O2
0.500 mol He
4.008 g H2
6.02 x 1023 molecules of N2
11.21
Which of the following samples occupy the largest
volume at STP? Note: R = 0.0821 L·atm/(mol·K).
1.
2.
3.
4.
5.
Tro IC3
1.00 mol O2
48.0 g O2
0.500 mol He
4.008 g H2
6.02 x 1023 molecules of N2
11.22
For an ideal gas, which two variables are
INVERSELY proportional to each other, assuming
all the other conditions remain constant?
1.
2.
3.
4.
5.
Tro IC3
V and P
T and P
V and T
V and n
None of the above
11.22
For an ideal gas, which two variables are
INVERSELY proportional to each other, assuming
all the other conditions remain constant?
1.
2.
3.
4.
5.
Tro IC3
V and P
T and P
V and T
V and n
None of the above
11.23
When the Celsius temperature of a gas sample is
doubled from 75 °C to 150 °C, the volume of the
gas:
(Assume the pressure is constant.)
1.
2.
3.
4.
5.
Tro IC3
Increases by a factor of 75
Halves
Doubles
Remains the same
None of the above
11.23
When the Celsius temperature of a gas sample is
doubled from 75 °C to 150 °C, the volume of the
gas:
(Assume the pressure is constant.)
1.
2.
3.
4.
5.
Tro IC3
Increases by a factor of 75
Halves
Doubles
Remains the same
None of the above
11.24
Which of the following gas laws relate volume and
temperature?
1.
2.
3.
4.
5.
Tro IC3
Avogadro’s law
Boyle’s law
Charles’s law
Gay-Lussac’s law
Dalton’s Law
11.24
Which of the following gas laws relate volume and
temperature?
1.
2.
3.
4.
5.
Tro IC3
Avogadro’s law
Boyle’s law
Charles’s law
Gay-Lussac’s law
Dalton’s Law
11.25
What is the SI unit for pressure?
1.
2.
3.
4.
5.
Tro IC3
Pa
atm
mm Hg
torr
psi
11.25
What is the SI unit for pressure?
1.
2.
3.
4.
5.
Tro IC3
Pa
atm
mm Hg
torr
psi