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Practice Exam 2 (CHEM 2045 UF)
Related Topics
Wize University Chemistry Textbook > Gases and their Properties
Other Applications of the Ideal Gas Law
6 Activities
Wize University Chemistry Textbook > Gases and their Properties
Ideal Gas Law
4 Activities
Consider two separate 1 L containers at 273 K, one filled with 2 g H
2
and one filled with 2 g of O
2.
Which of the following will be true?
Hydrogen gas will have a higher mass density
Hydrogen gas will have a higher pressure
Hydrogen gas will have a lower pressure
I don't know
Check Submission
More Other Applications of the Ideal Gas Law Questions:
Ideal Gas Law: Gas mixtures
When 100 g of Kr and 100 g of Xe are placed in a container, the partial pressure of Xe is found to be 4 atm. What is the partial pressure of Kr?
Ideal Gas Law: Gas mixtures
When 100 g of Kr and 100 g of Xe are placed in a container, the partial pressure of Xe is found to be 4 atm. What is the partial pressure of Kr?
Ideal Gas Law
If the following gases are used to fill balloons of a 1L volume at 1 atm and 298K, what is the correct ranking of the densities of the gases in the balloons.
C
H
4
\rm CH_4
C
H
4
,
C
2
H
6
\rm C_2H_6
C
2
H
6
,
C
4
H
10
\rm C_4H_{10}
C
4
H
10
,
X
e
\rm Xe
Xe
,
N
2
\rm N_2
N
2
,
O
2
\rm O_2
O
2
.
A 16.0 L gas vessel contains 40.0 kPa of He, 15.0 kPa of Ne and 25.0 kPa of Kr. What is the density of this mixture?
[Do NOT include units in your answers]
A mixture of gases containing 0
2
, N
2
and H
2
contains 0.20 mols of N
2
in a 12 L sealed vessel. If the total pressure is 188 kPa at 298 K, what is the partial pressure of nitrogen? What is the average molar mass of this mixture? The density of the mixture is 1.52g/L.
Ideal Gas Law
A 0.483 g sample of gas occupies a volume of 0.530 L at 130 °C and 109 kPa.
a. What is the molar mass of this gas?
b. Whats the density of this gas at STP?
Partial Pressure
300 mL H
2
was collected over water at 21
⁰
C and 748 Torr. Vapour pressure of water at 21
⁰
C is 18.65 Torr.
a. How many moles of H
2
and water vapour were present in the moist gas mixture?
b. Calculate the mass of the gas after being dried.
Vapor Pressure
A sample of H
2
gas was collected over water. The temperature of the vessel was 273.15 K and the volume of the sample was 20.0 L. The vapour pressure of water at 300.0 K is 5.0atm and the total pressure of the sample was 15.5atm. What is the mass of the H
2
in this sample?
What is the density of a sample of O
2
with a pressure of 1255 kPa at 10 °C?
Ideal Gas Laws
1. A mixture of gases containing O
2
, N
2
and H
2
contains 0.20 mols of N
2
in a 12 L sealed vessel. If the total pressure is 188 kPa at 298 K, what is the partial pressure of nitrogen? What is the average molar mass of this mixture? The density of the mixture is 1.52g/L.
Ideal Gas Laws
4. A 16.0 L gas vessel contains 40.0 kPa of He, 15.0 kPa of Ne and 25.0 kPa of Kr. What is the density of this mixture?
Ideal Gas Law
Calculate the density (in g/L) of HF gas at 35
o
C and 0.78 atm
Ideal Gas Law
Which of the following 5 gases has the lowest density at 50
o
C and 1.3 atm?
If the following gases are used to fill balloons of a 1L volume at 1 atm and 298K, what is the correct ranking of the densities of the gases in the balloons.
C
H
4
\rm CH_4
C
H
4
,
C
2
H
6
\rm C_2H_6
C
2
H
6
,
C
4
H
10
\rm C_4H_{10}
C
4
H
10
,
X
e
\rm Xe
Xe
,
N
2
\rm N_2
N
2
,
O
2
\rm O_2
O
2
.
Ideal Gas Law
7 moles of N
2
gas at 372 K was released into a 9 L balloon. If N
2
is a real gas, what is the pressure of the gas? (For N
2
,
a
= 0.0135 atm /L
2
, and
b
= 0.1937 L/mol, R = 0.08206 L*atm/mole*K).
Ideal Gas Law
0.238 g of a gas were placed in a 250 mL vessel. If the gas is heated to 85
o
C, the gas has a pressure of 7 atm. Which gas is in the vessel? (R = 0.08206 L*atm/mole*k)
"The Periodic Table", image retrieved from Chemistry 2e (https://d3bxy9euw4e147.cloudfront.net/oscms-prodcms/media/documents/Chemistry2e-OP_QCzV58S.pdf) by Flowers, P et al., is licensed under CC BY
Ideal Gas Law: Density
A 16.0 L gas vessel contains 40.0 kPa of He, 15.0 kPa of Ne and 25.0 kPa of Kr. What is the density of this mixture?
Ideal Gas Law
Consider the following 5 gases. If an equal volume of each gas is placed into a separate balloon, which gas sample will have the greatest mass? Assume the balloons are all at the same temperature and pressure.
A 6.00 L flask is evacuated and weighed, 21.64g. The vessel is then filled with a gas at STP, after filling the vessel weighs 27.31g. What is the molecular weight of the gas?
Ideal Gas Law: Identify the Ideal Gas
A scientist has a series of tubes filled with different noble gases in her lab. She realizes one day that the labels have worn away and she can't remember which gas is which. She decides to determine the gasses identity using the ideal gas law. She finds that there is 4.314 g of gas and at room temperature (298 K) the pressure in the 2.75 L tube is 97.4 kPa. What is the identity of the gas?
What is the density of a sample of O
2
with a pressure of 1255 kPa at 10 °C?
Molar Mass
A mixture of 5.5 mols of Ar, 3.5 mols of O
2
and 1.0 mol of Xe is prepared. What is the density of this mixture if the total pressure is 2.0 atm at 25° C?
Ideal Gas Law
A student has two balloons held at ambient pressure and temperature (1 atm, 298 K), one is 3 L contains Helium, the other is 14 L and contains argon. The student transfers both gasses into a single balloon which is also held at ambient temperature and pressure. What is the density of the gas mixture in the final balloon?
A mixture of ideal gases containing O
2
, F
2
and N
2
contains 0.20 mols of N
2
in a 12 L sealed vessel. If the density of this mixture is 1.52 g/L at room temperature under 188 kPa, of pressure. What is the average molar mass of this mixture?
Stoichiometry and Ideal Gas Law Practice
The combustion of methanol (CH
3
OH) is shown below. If 16g of methanol is burned in oxygen, what volume of CO
2
is produced if the pressure is 101.3kPa, T=25C, and R=8.314kPaL/molK? Round to the nearest whole number.
CH
3
OH + O
2
--> CO
2
+ H
2
O
Is the equation balanced?
No
A piece of zinc is allowed to react with an excess quantity of sulfuric acid, and the hydrogen gas produced is collected in a gas burette by displacement of water. Neglecting the effect of the vapor pressure of water on the system, calculate how many milligram (mg) of zinc would generate 92.0 mL of the gas at a temperature of 25.0 °C and a pressure of 1.00 atm.
At 150.°C and 1.00 atm, 500. mL of a vapor has a mass of 0.4183 g. What is the molecular weight of the compound?
Ideal Gas Law: Molecular weight
At 150.°C and 1.00 atm, 500. mL of a vapor has a mass of 0.4183 g. What is the molecular weight of the compound?
Gas Laws: Practice
A student decides to do a more controlled version of the hydrogen balloon explosion. The
unbalanced
chemical equation for this reaction is shown below:
H
2
(
g
)
+
O
2
(
g
)
→
H
2
O
(
g
)
H_2(g)+O_2(g)→H_2O(g)
H
2
(
g
)
+
O
2
(
g
)
→
H
2
O
(
g
)
(a)
Write the
balanced
chemical equation for this reaction.
Ideal Gas Law
A student adds 0.165 g of an unknown gas to a 125 mL flask. If the student finds the pressure to be 0.987 atm at 20.0 °C, is the gas likely to be methane, CH
4
, nitrogen, N
2
, oxygen, O
2
, neon, Ne , or argon, Ar?
More Ideal Gas Law Questions:
Ideal Gas Law: Kinetic Molecular Theory
The natural gas delivered to homes in Calgary is normally a mixture of methane (CH
4
), ethane (C
2
H
6
), propane (C
3
H
8
) and carbon dioxide (CO
2
).
(a)
In the laboratory, a chemistry student has collected some Calgarian natural gas in a 2.00 L plastic bottle at 0.902 atm and 23°C. What is the
concentration
of gas in the bottle?
(b)
The bottle was weighed before and after filling with gas to determine the exact composition of gases. The student found that in the mixture the mole fraction of C
3
H
8
(g) was 0.10 and the mole fraction of CH
4
(g) was 0.90. What was the
total mass of the gas
in the bottle?
Partial Pressure and Vapor Pressure
A sample of N
2
gas was collected over water. The temperature of the vessel was 300.0 K and the volume of the sample was 18.0 L. The vapor pressure of water at 300.0 K is 3.53 kPa and the total pressure of the sample was 122.00 kPa. What is the mass of the N
2
in this sample?
Practice: Kinetic Molecular Theory
The natural gas delivered to homes in Calgary is normally a mixture of methane (CH
4
), ethane (C
2
H
6
), propane (C
3
H
8
) and carbon dioxide (CO
2
).
(a)
In the laboratory, a CHEM 203 student has collected some Calgarian natural gas in a 2.00 L plastic bottle at 0.902 atm and 23°C. What is the
concentration
of gas in the bottle?
(b)
The bottle was weighed before and after filling with gas to determine the exact composition of gases. The student found that in the mixture the mole fraction of C
3
H
8
(g) was 0.10 and the mole fraction of CH
4
(g) was 0.90. What was the
total mass of the gas
in the bottle?
Ideal Gas Laws: Molar volume
Answer the following two questions based on the Ideal Gas Law:
Like Spring 2019 Exam 2
When 100 g of He and 100 g of Ne are placed in a container, the partial pressure of Ne is found to be 6 atm. What is the partial pressure of He?
Ideal Gas Law
If 10 g each of
O
2
(
g
)
\rm O_2(g)
O
2
(
g
)
and
H
B
r
(
g
)
\rm HBr(g)
HBr
(
g
)
are in separate containers of equal volume and temperature, which one of the following statements is true?
Partial Pressure and Vapor Pressure
A sample of N
2
gas was collected over water. The temperature of the vessel was 300.0 K and the volume of the sample was 18.0 L. The vapor pressure of water at 300.0 K is 3.53 kPa and the total pressure of the sample was 122.00 kPa. What is the mass of the N
2
in this sample?
Ideal Gas Law
4 moles of O
3(g)
are trapped inside a sealed rigid vessel. The gas undergoes a reaction,
O
3
(
g
)
→
1.5
O
2
(
g
)
\rm O_3(g) \rightarrow 1.5\ O_2(g)
O
3
(
g
)
→
1.5
O
2
(
g
)
Assuming all of the oxygen is consumed and the volume has remained constant, what was the effect on the pressure
A 10.0 L sample of Br
2
gas is collected over water at 298 K. If the total pressure of the sample is 180.0 kPa, how many mols of Br
2
are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa. [Do NOT include units in your answers]
A mixture of 4.6 mols of H
2
gas, 3.1 mols of N
2
gas and 2.6 mols of He are stored in a 60.0 L canister at 298 K. What is the partial pressure of each compound?
P
H
2
Find the new volume of 3.0 mols of an ideal gas initially at standard temperature and pressure after the pressure is changed to 40.0 kPa.
[Do Not include units in your answer]
Ideal vs real behaviour of gases
A sample of gas has a molar volume of 10.1 L at 745 Torr and −138
°
C. Is the gas behaving ideally?
Gas Stoichiometry and Limiting Reagent
Consider the following equation:
4NH
3
(g) + 7O
2
(g) → 4NO
2
(g) + 6H
2
O(l)
3 L NH
3
and 7 L O
2
were reacted at 350
°
C and 111 kPa. How much NO
2
can be produced?
Partial Pressure
A mixture of H
2
(g) and CO(g) (total mass 4.50 g) occupies a volume of 3.76 L at 298 K and 108 kPa. What is the partial pressure of each gas in this mixture? Calculate the volume percent of H
2
?
Vapour Pressure
A sample of N
2
gas was collected over water. The temperature of the vessel was 300.0 K and the volume of the sample was 18.0 L. The vapour pressure of water at 300.0 K is 3.53 kPa and the total pressure of the sample was 122.00 kPa. What is the mass of the N
2
in this sample?
Gas Law
Consider the following two containers of gas that are at the same temperature. Which of the following statements comparing these two containers are false and which are true?
Gases: Vapor Pressure
A sample of N
2
gas was collected over water. The temperature of the vessel was 300.0 K and the volume of the sample was 18.0 L. The vapour pressure of water at 300.0 K is 3.53 kPa and the total pressure of the sample was 122.00 kPa. What is the mass of the N
2
in this sample?
Ideal Gas Law: Gas Mixtures
2. A mixture of 4.6 mols of H
2
gas, 3.1 mols of N
2
gas and 2.6 mols of He are stored in a 60.0 L canister at 255 K. What is the partial pressure of each compound?
P
H
2
Ideal Gas Law: Gas Mixtures
3. A 10.0 L sample of Br
2
gas is collected over water at 298 K. If the total pressure of the sample is 180.0 kPa, how many mols of Br
2
are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa.
Ideal Gas Law: Partial Pressures
Calculate the partial pressure of neon (in atm) in a mixture of 3.1 g of argon, 1.2 g of neon, and 2.4 g of krypton at 0
o
C in 1.5 L container.
Ideal Gas Law: Pressure
0.103 moles of Cl
2
gas in a sealed cylinder with a piston has a volume of 3.25 L at a pressure of 0.780 atm. Assuming that the sample behaves as an ideal gas and the temperature remains constant, calculate the pressure (in atm) of the sample if the piston is moved and the volume of the cylinder is reduced to 1.82 L.
2 gases were mixed together in a 5 L vessel at 243 K to create a total pressure of 9.3 atm. If gas 1 has 2 moles, what is the partial pressure of gas 2? (R = 0.08206 L*atm/mole*K)
0.238 g of a gas were placed in a 250 mL vessel. If the gas is heated to 85
o
C, the gas has a pressure of 7 atm. Which gas is in the vessel? (R = 0.08206 L*atm/mole*k)
Ideal Gas Law: Molecular mass calculation
The density of an unknown gas at 100
o
C and 746 torr is 1.994 g/L. What is the molecular mass (in g/mol) of this unknown gas?
A mixture of 4.6 moles of H
2
gas, 3.1 moles of N
2
gas and 2.6 moles of He are stored in a 60.0 L canister at 298 K. What is the partial pressure of each compound? (Write answer in format X.XX atm, i.e. 4.25 atm)
P
H
2
3 moles of O
2
gas at 100 K was released into a 2 L balloon. If O
2
is a real gas, what is the pressure of the gas? (For O
2
,
a
= 0.0145 atm /L
2
, and
b
= 0.1711 L/mol, R = 0.08206 L*atm/mole*K).
An ideal gas at 30.0 C and pressure of 2 × 10
5
Pa is in a container having a volume of 1.40 L.
Determine the number of moles of gas in the container.
The gas pushes against a piston, expanding to twice its original volume, while the pressure falls to atmospheric pressure. Find the final temperature.
Ideal Gas Laws: Gas mixtures
2 gases were mixed together in a 5 L vessel at 243 K to create a total pressure of 9.3 atm. If gas 1 has 2 moles, what is the partial pressure of gas 2? (R = 0.08206 L*atm/mole*K)
Gas Laws: Van der Waals Equation
Find the difference between the ideal pressure and the Van der Waals pressure for 2 mol of CO
2
in a 1L vessel at room temperature. CO
2
(a = 3.640 L
2
atm/mol
2
; b = 0.04267 L/mol).
Ideal Gas Law
A sample of argon is loaded into a 3L sealed vessel and at room temperature the initial pressure is 2.6atm. The vessel is then loaded into an autoclave and heated to 580
o
C. What is the final pressure inside the vessel?
Ideal Gas Law
A 8.0 L sample of Br
2
gas is collected over water at 298 K. If the total pressure of the sample is 168.0 kPa, how many moles of Br2 are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa.
Ideal Gas Law: Partial Pressure
A mixture of 4.6 moles of H
2
gas, 3.1 moles of N
2
gas and 2.6 moles of He are stored in a 60.0 L canister at 255 K. What is the partial pressure of each compound?
P
H
2
Ideal Gas Law: Mole fraction
A 10.0 L sample of Br
2
gas is collected over water at 298 K. If the total pressure of the sample is 180.0 kPa, how many moles of Br
2
are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa.
Ideal Gas Law
A sample of a gaseous compound is distributed into two vessels, A and B, of equal volume held at the same temperature and pressure. Vessel A is heated to twice its initial temperature in Kelvin, followed by compression to one quarter of its initial volume. Vessel B is cooled to half of its initial temperature in K, followed by expansion to twice it’s original volume. What is the ratio of the pressure in vessel A to the pressure in vessel B after these transformations?
Ideal Gas Law: Volume as a function of pressure
Find the new volume of 3.0 moles of an ideal gas initially at standard temperature and pressure after the pressure is changed to 40.0 kPa.
Ideal Gas Law: Volume as a function of moles
What is the volume of 2.5 moles of Ne at 298 K and 1.0 atm? What is the new volume after 4.5 moles of Ne are added?
Ideal Gas Law: Gas mixtures
A mass of 0.4 g of hydrogen (H
2
) and 3.2 g of helium (He) are mixed in a rigid 500 mL container. What is the partial pressure of helium when the container is cooled to 77 K?
A 6.00 L flask is evacuated and weighed, 21.64g. The vessel is then filled with a gas at STP, after filling the vessel weighs 27.31g. What is the molecular weight of the gas?
Ideal Gas Law: Identify the Ideal Gas
A scientist has a series of tubes filled with different noble gases in her lab. She realizes one day that the labels have worn away and she can't remember which gas is which. She decides to determine the gasses identity using the ideal gas law. She finds that there is 4.314 g of gas and at room temperature (298 K) the pressure in the 2.75 L tube is 97.4 kPa. What is the identity of the gas?
Practice: Ideal Gas Law
3.0 moles of Argon are stored in a 2.0 L container kept at 10 °C. What is the pressure of this gas? Please calculate the pressure in kPa.
A sample of a gaseous compound is distributed into two vessels, A and B, of equal volume held at the same temperature and pressure. Vessel A is heated to twice its initial temperature in Kelvin, followed by compression to one quarter of its initial volume. Vessel B is cooled to half of its initial temperature in K, followed by expansion to twice it’s original volume. What is the ratio of the pressure in vessel A to the pressure in vessel B after these transformations?
A 15 L sample of N
2
gas held at 328 K is compressed such that the pressure rises from 1.0 atm to 7.8 atm. What is the final volume of the gas?
For an ideal gas which variables in the following pairs are not directly proportional to each other (if all other factors remain constant)?
Find the new volume of 3.0 mols of an ideal gas initially at standard temperature and pressure after the pressure is dropped to 20.0 kPa.
When coal is burned, sulfur that is present within coal is converted to sulfur dioxide (SO
2
). This results in the acid rain phenomenon. If 3.75 kg of S are reacted with oxygen, calculate the volume of SO
2
gas (in L) formed at 25.0 °C and 1.10 atm.
Ideal Gas Law: Stoichiometry
What volume of hydrogen (STP) is produced by dissolving one-half mole of aluminum in sulfuric acid?
2
A
l
(
s
)
+
3
H
2
S
O
4
(
a
q
)
→
A
l
2
(
S
O
4
)
3
(
a
q
)
+
3
H
2
(
g
)
2Al(s)+3H_2SO_4(aq)→Al_2(SO_4)_3(aq)+3H_2(g)
2
A
l
(
s
)
+
3
H
2
S
O
4
(
a
q
)
→
A
l
2
(
S
O
4
)
3
(
a
q
)
+
3
H
2
(
g
)
Ideal Gas Law: Molecular weight
At 150.°C and 1.00 atm, 500. mL of a vapor has a mass of 0.4183 g. What is the molecular weight of the compound?
Which of the following graphs is
NOT
consistent with the ideal gas law assuming that the other parameters are kept constant?
Ideal Gas Law: Practice
A small tank of compressed oxygen gas is left outside in the sun and its temperature increases.
Assume that the amount of gas and the volume of the tank do not change
.
Identify which of the four graphs below show how…
A. …the pressure (P) of the gas inside the tank changes as T increases.
Ideal Gas Law: Kinetic Molecular Theory
The natural gas delivered to homes in Calgary is normally a mixture of methane (CH
4
), ethane (C
2
H
6
), propane (C
3
H
8
) and carbon dioxide (CO
2
).
(a)
In the laboratory, a chemistry student has collected some Calgarian natural gas in a 2.00 L plastic bottle at 0.902 atm and 23°C. What is the
concentration
of gas in the bottle?
(b)
The bottle was weighed before and after filling with gas to determine the exact composition of gases. The student found that in the mixture the mole fraction of C
3
H
8
(g) was 0.10 and the mole fraction of CH
4
(g) was 0.90. What was the
total mass of the gas
in the bottle?
The enthalpy of combustion for ethanol (C
2
H
5
OH) is -1370.7 kJ/mol. Calculate q, w, ΔH and ΔU when 45g of ethanol are burned at 1atm and 298K.
Stoichiometry
The following gaseous reaction takes place at 473 K and 101.3 kPa:
N
2
(
g
)
+
O
2
(
g
)
→
N
O
2
(
g
)
N_{2(g)}+O_{2(g)}\to NO_{2(g)}
N
2
(
g
)
+
O
2
(
g
)
→
N
O
2
(
g
)
If 80.0 g of 0
2
are available to react, how many litres of N
2
will be required to completely consume the oxygen supply?
Ideal Gas Laws
5. Find the new volume of 3.0 mols of an ideal gas initially at standard temperature and pressure after the pressure is changed to 40.0 kPa.
Ideal Gas Laws: Volume
6. What is the volume of 2.5 mols of Ne at 298 K and 1.0 atm? What is the new volume after 4.5 mols of Ne are added?
Worked Example
Four moles of an ideal gas originally at 323
o
C and 7.3 atm underwent a complete expansion against a constant external pressure of 1 atm and did 8kJ of work. Calculate q, ΔE, ΔH.
Solve for the missing initial variable (Vi):
hint: rearrange PV=nRT to do this!
Ideal Gas law
Inflatable balloons are often used to gently lift a sunken ship from the ocean floor to the ocean surface. We want to fill two balloons (one for each side of the ship) that are approximately 100m long cylinders with a radius of 0.5m with nitrogen gas at a pressure of 1.1 atm. If we remember that the water temperature at the ocean floor is approximately 0
o
C how much nitrogen will we need? Answer in moles. R=0.08206Latm/Kmol
Ideal Gas Law
1.1 mols of Argon are stored in a 2.0 L container kept at 10 °C. What is the pressure of this gas? (answer in kPa)
Like Spring 2019 Exam 2
At 100
o
C and 1.00 atm, what volume of nitrogen gas is required to react completely with 10.0 L of hydrogen gas to produce ammonia gas?
Ideal Gas Law
12 moles of Xenon are held inside a 15L flask at room temperature.
The flask is then cooled to – 100
o
C.The flask is then allowed to expand into a 23L but we need to keep the pressure constant. What temperature is required to keep the pressure constant as the gas expands into the new volume.
Ideal Gas Law
12 moles of Xenon are held inside a 15L flask at room temperature.
The flask is then cooled to – 100
o
C what is the pressure inside the flask at -100
o
C?
Ideal Gas Law
12 moles of Xenon are held inside a 15L flask at room temperature.
What is the initial pressure inside the flask?
Ideal Gas Law
Four grams of Helium (an ideal gas) is packed into a 500mL flask and heated in a boiling pot of water. What is the internal pressure of the flask? R=0.08206Latm/Kmol