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Ideal Gas Laws: Molar volume
Related Topics
Wize University Chemistry Textbook > Gases and their Properties
Ideal Gas Law
4 Activities
Wize University Chemistry Textbook > Gases and their Properties
Gas Laws
4 Activities
Answer the following two questions based on the Ideal Gas Law:
Part 1
Part 2
What is the volume of 2.5mol of Ne at 298K and 101.325kPa?
Enter your answer to one decimal point and make sure to include units.
Answer
I don't know
Previous Part
Check Part 1
Next Part
Check Submission
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?
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)
Practice Exam 2 (CHEM 2045 UF)
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?
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
More Gas Laws Questions:
Gases
In the gas apparatus below, the pressure of the gas in the 5.0 L bulb is 1 atm and the pressure of the gas in the 2.0 L bulb is 3.0 atm. What is the pressure in the bulbs once the valve is opened, assuming the temperature is held constant.
Gases
In the gas apparatus below, the pressure of the gas in the 5.0 L bulb is 1 atm and the pressure of the gas in the 2.0 L bulb is 3.0 atm. What is the pressure in the bulbs once the valve is opened, assuming the temperature is held constant.
Gas Laws: Kinetic energy
Which of the following relationships is/are CORRECT for gases?
Ideal Gas Law
Which of the following changes will NOT affect the total pressure of gas in a container, assuming all other factors remain constant?
Gas Mixtures: Partial pressures
Consider the gas-phase reaction shown in this balanced chemical equation:
2
A
(
g
)
+
B
2
(
g
)
→
2
A
B
(
g
)
2A(g)+B_2(g)→2AB (g)
2
A
(
g
)
+
B
2
(
g
)
→
2
A
B
(
g
)
A rigid flask is filled with gases so that the initial partial pressure of A is 1.0 atm and the intial partial pressure of B is 0.50 atm. If the reaction goes to completion and the temperature stays constant, what is the final pressure in the flask?
Ideal Gas Laws
At very high pressures, gas properties deviate from those predicted by the ideal gas law. The actual volume of the gas will be…
Gas Laws
Suppose you have a sample of gas at a fixed temperature, and you increase the volume of the container. The pressure changes, since there are...
Gas Laws
Which of the following relationships is/are CORRECT for gases?
The amount of a gas (in moles) is inversely proportional to its volume (at constant temperature and pressure).
The volume of a gas is directly proportional to its temperature in kelvin (at constant pressure and moles).
2 moles of hydrogen gas are held in a sealed steel vessel so that the Volume is held constant. The temperature is doubled, what is the effect on the pressure?
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?
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?
Whose law states that at constant temperature for a fixed amount of gas, the volume is inversely proportional to the pressure?
Who is the scientist who related the volume of gas to the number of particles contained in the gas, regardless of which gas it is?
Gas Law: Volume
If the pressure inside a container is kept constant and the container is heated, what would happen to the volume of the gas?
Gases (Ideal)
A tank of gas has a pressure of 10 atm at 25
o
C. At what temperature (in degrees Celcius) will it reach a pressure of 20 atm?
Gas Laws: Pressure as a function of temperature
An ideal gas is heated in a sealed container from 45 °C to 100 °C. If the original pressure in the vessel was 0.50 atm, what is the pressure after heating in kPa?
Gas Laws
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?
If there are 0.33 moles each of hydrogen (H
2
), argon (Ar), and methane (CH
4
) at the same temperature and pressure then which statement is CORRECT?
To increase the volume of a fixed amount of gas from 100 mL to 200 mL
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)?
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: Mixtures of Gases
You have a rigid container filled with a mixture of three gases: nitrogen, oxygen, and carbon dioxide. Your task is to compare two different methods to remove all of the carbon dioxide from the container.
Method
A:
Adding a solid material which
adsorbs
CO
2
gas – this means that CO
2
molecules stick to this material so that all of the CO
2
will be removed when the solid is removed.
Method
B:
Adding an excess of solid sodium peroxide (Na
2
O
2
) to convert all of the CO
2
gas to oxygen gas.
Gas laws
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?
Gas Laws: Pressure
4. 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 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?
Gas Stoichiometry
A tank of gas has a pressure of 5 atm at 25
o
C. At what temperature (in degrees Celsius) will it reach a pressure of 8 atm?
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?
Gases
In the gas apparatus below, the pressure of the gas in the 5.0 L bulb is 1 atm and the pressure of the gas in the 2.0 L bulb is 3.0 atm. What is the pressure in the bulbs once the valve is opened, assuming the temperature is held constant.