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

12 moles of Xenon are held inside a 15L flask at room temperature.

What is the initial pressure inside the flask?

12 moles of Xenon are held inside a 15L flask at room temperature.

The flask is then cooled to – 100oC what is the pressure inside the flask at -100oC?

12 moles of Xenon are held inside a 15L flask at room temperature.

The flask is then cooled to – 100oC.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.

At 100oC 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?

Consider two separate 1 L containers at 273 K, one filled with 2 g H2 and one filled with 2 g of O2. Which of the following will be true?

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)

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 oC how much nitrogen will we need? Answer in moles. R=0.08206Latm/Kmol

Four moles of an ideal gas originally at 323 oC 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!

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?

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.

The following gaseous reaction takes place at 473 K and 101.3 kPa:

$N_{2(g)}+O_{2(g)}\to NO_{2(g)}$

If 80.0 g of 02 are available to react, how many litres of N2 will be required to completely consume the oxygen supply?

The enthalpy of combustion for ethanol (C2H5OH) is -1370.7 kJ/mol. Calculate q, w, ΔH and ΔU when 45g of ethanol are burned at 1atm and 298K.

The natural gas delivered to homes in Calgary is normally a mixture of methane (CH4), ethane (C2H6), propane (C3H8) and carbon dioxide (CO2).

(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 C3H8(g) was 0.10 and the mole fraction of CH4(g) was 0.90. What was the total mass of the gas in the bottle?

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.

Which of the following graphs is NOT consistent with the ideal gas law assuming that the other parameters are kept constant?

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?

What volume of hydrogen (STP) is produced by dissolving one-half mole of aluminum in sulfuric acid?

$2Al(s)+3H_2SO_4(aq)→Al_2(SO_4)_3(aq)+3H_2(g)$

When coal is burned, sulfur that is present within coal is converted to sulfur dioxide (SO2). This results in the acid rain phenomenon. If 3.75 kg of S are reacted with oxygen, calculate the volume of SO2 gas (in L) formed at 25.0 °C and 1.10 atm.

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.

For an ideal gas which variables in the following pairs are not directly proportional to each other (if all other factors remain constant)?

A 15 L sample of N2 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?

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?

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 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?

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?

A mass of 0.4 g of hydrogen (H2) 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?

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?

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.

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 10.0 L sample of Br2 gas is collected over water at 298 K. If the total pressure of the sample is 180.0 kPa, how many moles of Br2 are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa.

A mixture of 4.6 moles of H2 gas, 3.1 moles of N2 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?

1. P
2. H2

A 8.0 L sample of Br2 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.

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 580oC. What is the final pressure inside the vessel?

Find the difference between the ideal pressure and the Van der Waals pressure for 2 mol of CO2 in a 1L vessel at room temperature. CO2 (a = 3.640 L2atm/mol2; b = 0.04267 L/mol).

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)

If 10 g each of $\rm O_2(g)$ and $\rm HBr(g)$ are in separate containers of equal volume and temperature, which one of the following statements is true?

An ideal gas at 30.0 C and pressure of 2 × 105 Pa is in a container having a volume of 1.40 L.

1. Determine the number of moles of gas in the container.
2. The gas pushes against a piston, expanding to twice its original volume, while the pressure falls to atmospheric pressure. Find the final temperature.

3 moles of O2 gas at 100 K was released into a 2 L balloon. If O2 is a real gas, what is the pressure of the gas? (For O2, a = 0.0145 atm /L2, and b = 0.1711 L/mol, R = 0.08206 L*atm/mole*K).

A mixture of 4.6 moles of H2 gas, 3.1 moles of N2 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)

1. P
2. H2

The density of an unknown gas at 100oC and 746 torr is 1.994 g/L. What is the molecular mass (in g/mol) of this unknown gas?

0.238 g of a gas were placed in a 250 mL vessel. If the gas is heated to 85 oC, the gas has a pressure of 7 atm. Which gas is in the vessel? (R = 0.08206 L*atm/mole*k)

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)

0.103 moles of Cl2 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.

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 0oC in 1.5 L container.

3. A 10.0 L sample of Br2 gas is collected over water at 298 K. If the total pressure of the sample is 180.0 kPa, how many mols of Br2 are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa.

2. A mixture of 4.6 mols of H2 gas, 3.1 mols of N2 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?

1. P
2. H2

A sample of N2 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 N2 in this sample?

A sample of N2 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 N2 in this sample?

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?

A sample of N2 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 N2 in this sample?

A mixture of H2(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 H2?

Consider the following equation:

4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(l)

3 L NH3 and 7 L O2 were reacted at 350 °C and 111 kPa. How much NO2 can be produced?

A sample of gas has a molar volume of 10.1 L at 745 Torr and −138 °C. Is the gas behaving ideally?

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]

A mixture of 4.6 mols of H2 gas, 3.1 mols of N2 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?

1. P
2. H2

A 10.0 L sample of Br2 gas is collected over water at 298 K. If the total pressure of the sample is 180.0 kPa, how many mols of Br2 are present in this sample? The vapor pressure of water at 298 K is 3.17 kPa. [Do NOT include units in your answers]

4 moles of O3(g) are trapped inside a sealed rigid vessel. The gas undergoes a reaction,

$\rm O_3(g) \rightarrow 1.5\ O_2(g)$

Assuming all of the oxygen is consumed and the volume has remained constant, what was the effect on the pressure

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?

Answer the following two questions based on the Ideal Gas Law:

The natural gas delivered to homes in Calgary is normally a mixture of methane (CH4), ethane (C2H6), propane (C3H8) and carbon dioxide (CO2).

(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 C3H8(g) was 0.10 and the mole fraction of CH4(g) was 0.90. What was the total mass of the gas in the bottle?

A sample of N2 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 N2 in this sample?

The natural gas delivered to homes in Calgary is normally a mixture of methane (CH4), ethane (C2H6), propane (C3H8) and carbon dioxide (CO2).

(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 C3H8(g) was 0.10 and the mole fraction of CH4(g) was 0.90. What was the total mass of the gas in the bottle?