Practice: A gas mixture with a total pressure of 812 mmHg contains the following gases at with their partial pressures: Cl_{2 }= 210 mmHg, H_{2} = 180 mmHg, CO_{2} = 215 mmHg. If argon gas is also present calculate its mole fraction.

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According to Dalton’s Law, the **total pressure** inside a container is obtained by adding all the **partial pressures** of each non-reacting gas.

Concept #1: Understanding Dalton's Law

**Transcript**

Welcome back guys. In this video, we're going to take a look at the partial pressure of gases. Now, what do I mean by partial pressure? What we said in the beginning, that pressure equals force over area. We saw a picture of the container with several different types of gas particles. We're going to say that the total pressure inside of that container comes from all the pressures that each of those particles added up.

Let's say we wanted to look at the pressure of one of those gas particles and ignore the others. The pressure of that one single gas particle would be that gas particles partial pressure. It just means the pressure of a gas when it surrounded by a bunch of different gases. We're not looking at the total pressure. We're looking at that gas particles individual pressure. That individual pressure is partial pressure.

We're going to say Dalton's law states that, 'In a container of unreacting gases,' that means that these gases are just bouncing off of each other. They're not connecting together to give me a new compound. 'The total pressure of the container is the sum of the partial pressure of the individual gases.' All these mean is let's say we have a container and its filled with three types of gases. It's filled with O2, argon and neon gas.

Let's say that the pressure of the oxygen gas is 0.3 atm and argon is 0.1 atm and neon is 0.3 atm. We'd say that each of them has those individual pressures—that's their partial pressures. Dalton's law says, while the total pressure inside of the container is just each of them added up together. According to Dalton's law, the total pressure equals 0.7 atm, and that 0.7 atm comes from us adding up each of those individual pressures together.

Concept #2: Understanding mole fraction and partial pressure

**Transcript**

We're going to say that the total pressure due like we said to the total number of moles of each of these gas particles. So pressure and moles are connected together. We're going to say the partial pressure of each gas molecule is a total pressure multiplied by the mole fraction of each gas particle or gas molecule. What the heck does that mean?

What I'm saying here is, the pressure of a gas, of any individual gas is equal to its mole fraction, mole fraction is X. We're going to say, 'What the heck is mole fraction?' Mole fraction is the moles of that gas divided by the total moles of all the gases. If we're looking for example the mole fraction of neon gas, it'd be the moles of neon divided by the moles of oxygen, argon plus neon on the bottom. That would give us the mole fraction of neon.

Once we get the mole fraction of a gas, we would multiply times the total pressure. That would then give me just the pressure of that one gas. Here this is just partial pressure. I know these ideas are kind of abstract, so that's why we're going to move on to the next question, the example. This is going to show us how exactly does, how do we find the partial pressure of the gas and does that relate to the mole fraction of that gas.

The **partial pressure** of a gas is based on the moles of that gas. The relationship of the different moles of gases helps us determine the **mole fraction** of each gas.

Example #1: A container has 16.7 g O_{2}, 8.1 g H_{2} and 35.2 g N_{2} and contains a total pressure of 0.83 atm. Calculate the mole fraction of O_{2} and its partial pressure.

Practice: A gas mixture with a total pressure of 812 mmHg contains the following gases at with their partial pressures: Cl_{2 }= 210 mmHg, H_{2} = 180 mmHg, CO_{2} = 215 mmHg. If argon gas is also present calculate its mole fraction.

A mixture of He and O2 is placed in a 4 L flask at 300 K. The partial pressure of the He is 2.7 atm and the partial pressure of the O2 is 1.4 atm. What is the mole fraction of O 2?
a. 0.341
b. 0.481
c. 0.518
d. 0.659
e. 0.224

A flask at equilibrium contained 1.00 mol of N 2 gas, 2.00 mol of H2 gas, and 3.00 mol of He gas. The total pressure in the container was 1.00 atm. What was the partial pressure of the He gas in torr?
a) none of the given answers
b) 380
c) 2280
d) 760
e) 4560

A gaseous mixture containing 1.5 mol Ar and 3.5 mol CO 2 has a total pressure of 7.0 atm. What is the partial pressure of CO2?
a) 1.8 atm
b) 2.1 atm
c) 3.5 atm
d) 4.9 atm
e) 2.4 atm

A mixture of N 2, O2 and Ar have mole fractions of 0.25, 0.65, and 0.10, respectively. What is the pressure of N2 if the total pressure of the mixture is 3.9 atm?
A) 2.5 atm
B) 0.39 atm
C) 0.67 atm
D) 0.98 atm
E) 1.33 atm

A mixture of oxygen and helium is 92.3% by mass oxygen. It is collected at atmospheric pressure (687 torr). What is the partial pressure of oxygen in this mixture?
1. 446 Torr
2. 414 Torr
3. 688 Torr
4. 299 Torr
5. 333 Torr

A mixture of CO, CO2 and O2 is contained within a 275 mL flask at 0°C. if the total pressure is 780 torr, the CO has a partial pressure of 330 torr and the CO2 has a partial pressure of 330 torr, what is the partial pressure of O2?
1. 330 torr
2. 900 torr
3. 120 torr
4. 780 torr
5. 660 torr

A vessel contains 0.1 mol H2 gas, 0.1 mol N2 gas, and 0.3 mol NH3 gas. The total pressure is 1000 torr. What is the partial pressure of
the H2 gas?
1. 1000 torr
2. 500 torr
3. 100 torr
4. 800 torr
5. 200 torr

The partial pressure of an ideal gas is equal to:
a. The pressure it would exert if it were at high pressure, same volume, and alone in a container
b. The pressure it would exert if it were at low pressure, same volume, and alone in a container.
c. The pressure it would exert if it occupied the same volume, alone in a container, at the same temperature.
d. The pressure it would exert if it were at low temperature, same volume, and alone in a container.
e. The pressure it would exert if it were at high temperature, same volume, and alone in a container.

A gaseous mixture of O 2 and N2 contains 39.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 505 mmHg?
a. 171 mmHg
b. 60 mmHg
c. 870 mmHg
d. 288 mmHg
e. 700 mmHg

What is the vapor pressure of a solution with a benzene to octane molar ratio of 2:1?
(A) 120 mmHg
(B) 320 mmHg
(C) 400 mmHg
(D) 680 mmHg

A mixture of He and O 2 is placed in a 4 L flask at 300 K. The partial pressure of the He is 2.7 atm and the partial pressure of the O2 is 1.4 atm. What is the mole fraction of O 2?
a. 0.341
b. 0.481
c. 0.518
d. 0.659
e. 0.224

A 100 L balloon is blown up with a mixture of gases. The mixture contains 2.1 moles of oxygen, 3.5 moles of nitrogen, and 1.8 moles of helium. Find the partial pressure for the oxygen if the balloon is at atmposheric pressure.
a. 0.28 atm
b. 0.47 atm
c. 0.24 atm
d. 0.22 atm
e. 0.78 atm

A mixture of 0.50 moles of Ne and 0.25 moles of Ar has a total pressure of 1.6 atm. What is the partial pressure (in atm) of Ne?
A. 1.1 atm
B. 1.3 atm
C. 0.40 atm
D. 0.80 atm
E. 0.54 atm

A mixture of 10.0 g of Ne and 10.0 g Ar have a total pressure of 1.6 atm. What is the partial pressure of Ne?
A) 1.3 atm
B) 1.1 atm
C) 0.80 atm
D) 0.40 atm
E) 0.54 atm

A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm?

A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon.
a. Which of the two gases exerts the greater partial pressure?

A mixture of 0.220 moles CO, 0.350 moles H 2 and 0.640 moles He has a total pressure of 2.95 atm. What is the pressure of H2 (in atm)?a. 1.56 atmb. 0.649 atmc. 1.03 atmd. 0.853 atm

Determine the vapor pressure of a solution at 25°C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapor pressure of pure water at 25°C is 23.8 torr. (Density of water is 1.0 g/mL)A) 70.8 torrB) 72.9 torrC) 23.1 torrD) 22.9 torrE) 7.29 torr

Calculate the vapor pressure at 25◦C of a mixture of benzene and toluene in which the mole fraction of benzene is 0.650. The vapor pressure at 25◦C of benzene is 94.6 torr and that of toluene is 29.1 torr.a. 51.3 torrb. 61.5 torrc. 84.4 torrd. 124 torre. 71.7 torr

Chloroform and methanol form an ideal solution. The solution boils at 22°C and 0.255 atm. At 22°C the vapor pressures of methanol and chloroform are 0.192 atm and 0.311 atm respectively. What is the mole fraction of chloroform in the solution?

A solution contains a mixture of pentane and hexane at room temperature. The solution has a vapor pressure of 256 torr. Pure pentane and hexane have vapor pressures of 425 torr and 151 torr, respectively, at room temperature.
What is the mole fraction of hexane? (Assume ideal behavior.)

A gas mixture contains an equal number of moles of He and Ne. The total pressure of the mixture is 6.0 atm .What is the partial pressure of He?

Consider the following samples of gases:If the three samples are all at the same temperature, rank them with respect to total pressure (Pt).

A 1.00-L gas sample at 100.°C and 600. torr contains 50.0% helium and 50.0% xenon by mass. What are the partial pressures of the individual gases?

Consider the flasks in the following diagrams.b. Assuming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened.

Three equal volumes of gas mixtures, all at the same T, are depicted below (with gas A red, gas B green, and gas C blue):(a) Which sample, if any, has the highest partial pressure of A?

A gaseous mixture of O 2 and N2 contains 40.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 585 mmHg ?

A mixture of CO2 and Kr weighs 35.0 g and exerts a pressure of 0.708 atm in its container. Since Kr is expensive, you wish to recover it from the mixture. After the CO2 is completely removed by absorption with NaOH(s), the pressure in the container is 0.250 atm. How many grams of CO2 were originally present? How many grams of Kr can you recover?

Assume that an exhaled breath of air consists of 74.7 % N2, 15.4 % O2, 3.8 % CO2, and 6.1 % water vapor.If the total pressure of the gases is 0.990 atm , calculate the partial pressure of O2.

Consider the flasks in the following diagrams.c. Solve for the final pressure in terms of the original pressures of helium and neon. Assume temperature is constant.

A 36.0–L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO2, 805 g O2, and 4,880 g N2. At 25 degrees C, what is the pressure in the cylinder in atmospheres?

Containers A, B, and C are attached by closed stopcocks of negligible volume.If each particle shown in the picture represents 106 particles, (c) If the pressure in C, PC, is 750 torr before the stopcocks are opened, what is PC afterward?

A 2.00-L sample of O2(g) was collected over water at a total pressure of 785 torr and 25°C. When the O2(g) was dried (water vapor removed), the gas had a volume of 1.94 L at 25°C and 785 torr. Calculate the vapor pressure of water at 25°C.

Determine the partial pressure of each gas as shown in the figure below. Note: The relative numbers of each type of gas are depicted in the figure.

Consider the flask apparatus below, which now contains 2.00 L H 2 at a pressure of 360. torr and 1.00 L N2 at an unknown pressure. If the total pressure in the flasks is 320. torr after the stopcock is opened, determine the initial pressure of N2 in the 1.00-L flask.

A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 torr. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)

In a system for separating gases a tank containing a mixture of hydrogen and carbon dioxide is connected to a much larger tank where the pressure is kept very low. The two tanks are separated by a porous membrane through which the molecules must effuse. If the initial partial pressures of each gas is 5.00 atm, what will be the mole fraction of hydrogen in the tank after the partial pressure of carbon dioxide has declined to 4.50 atm?

What is the mole fraction of H2 in a mixture of 15.1 g of O2, 8.18 g of N2, and 2.47 g of H2?

At 20 oC the vapor pressure of benzene C6H6 is 75 torr and that of toluene C7H8 is 22 torr. Assume that benzene and toluene form an ideal solution.In a solution composed of benzene and toluene that has a vapor pressure of 36 torr at 20 oC, what is the mole fraction of toluene?

An equimolar mixture of Ne and Xe is accidentally placed in a container that has a tiny leak. After a short while, a very small proportion of the mixture has escaped. What is the mole fraction of Ne in the effusing gas?

Chlorine gas reacts with fluorine gas to form chlorine trifluoride.
Cl2(g) + 3F2(g) → 2ClF3(g)
A 2.00 L reaction vessel, initially at 298 K, contains chlorine gas at a partial pressure of 337 mmHg and fluorine gas at a partial pressure of 784 mmHg .
a. What is the pressure of ClF3 in the reaction vessel after the reaction?
b. What is the total pressure in the reaction vessel after the reaction?

The atmospheric concentration of CO2 gas is presently 390 ppm (parts per million, by volume; that is, 390 L of every 106 L of the atmosphere are CO2).What is the mole fraction of CO2 in the atmosphere?

How is the partial pressure exerted by N2 gas affected when some O2 is introduced into a container if the temperature and volume remain constant?

During a persons typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume.Calculate the partial pressure of the CO2 in the expired air at its peak, assuming 1 atm pressure and a body temperature of 37oC .

Air is about 78.0% nitrogen molecules and 21.0% oxygen molecules. Several other gases make up the remaining 1% of air molecules. What is the partial pressure of nitrogen in air at atmospheric pressure (1.0 atm)?

A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.2 atm?

Consider a mixture of two gases, A and B, confined in a closed vessel. A quantity of a third gas, C, is added to the same vessel at the same temperature. How does the addition of gas C affect the following?the mole fraction of gas B

At 63.5oC the vapor pressure of H2O is 175 torr, and that of ethanol (C2H5OH) is 400 torr. A solution is made by mixing equal masses of H2O and C2H5OH.What is the mole fraction of ethanol in the vapor above the solution?

A gas mixture contains an equal number of moles of He and Ne. The total pressure of the mixture is 6.0 atm .What is the partial pressure of Ne?

Consider a mixture of two gases, A and B, confined in a closed vessel. A quantity of a third gas, C, is added to the same vessel at the same temperature. How does the addition of gas C affect the following.The partial pressure of gas A

Consider this molecular-level representation of a gas.If the partial pressure of the diatomic gas is 0.480 atm, what is the total pressure?

Consider this molecular-level representation of a gas.If the partial pressure of the diatomic gas is 0.810 atm, what is the total pressure?

A sample of 1.43 g of helium and an unweighed quantity of O2 are mixed in a flask at room temperature. The partial pressure of helium in the flask is 43.0 torr , and the partial pressure of oxygen is 158 torr .What is the mass of the oxygen in the container?

Calculate the vapor pressure (in torr) at 298 K in a solution prepared by dissolving 32 g of the non-volatile non-electrolye glucose in 186 g of methanol. The vapor pressure of methanol at 298 K is 122.7 torr. Enter your answer to 2 decimal places.a. 97.06 torrb. 119.06 torrc. 149.2 torrd. 24.8 torre. 21.14 torr

A mixture of CH4 (g) and C2 H6 (g) has a total pressure of 0.54 atm . Just enough O2 (g) is added to the mixture to bring about its complete combustion to CO2 (g) and H2 O(g). The total pressure of the two product gases is 2.3 atm .Assuming constant volume and temperature, find the mole fraction of CH4 in the mixture.

A mixture of three gases has a pressure of 1380 mmHg at 298 K. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar? a. 238 mm Hg b. 302 mm Hg c. 356 mm Hg d. 1753 mm Hg e. 8018 mm Hg

A gas sample contains 3.50 moles of argon, 2.08 moles of neon and 1.22 moles of nitrogen. If the total pressure of the sample is 3.66 atm, what is the partial pressure of argon?(A) 3.66 atm (B) 22.4 atm (C) 0.179 atm (D) 1.12 atm (E) 1.88 atm

A mixture of 10.0 g of Ne and 10.0 g of Ar has a total pressure of 1.6 atm. What is the partial pressure of Ne?a. 1.1 atmb. 0.8 atmc. 0.54 atmd. 0.40 atme. 1.3 atm

In a mixture of N 2 and O2 gases, the mol fraction of N 2 is found to be 0.700. The total pressure of the mixture is 1.42 atm. What is the partial pressure of O2 in the mixture?a) 0.211 atmb) 0.426 atmc) 0.493 atmd) 0.994 atm

A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium.What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.6 atm ?

A mixture of 8.1 g CH4 and 8.1 g Xe is placed in a container and the total pressure is found to be 0.45 atm .Find the partial pressure of CH4.

Assume that an exhaled breath of air consists of 74.7 % N2, 15.4 % O2, 3.8 % CO2, and 6.1 % water vapor.If the total pressure of the gases is 0.990 atm , calculate the partial pressure of water vapor.

A sample of gas isolated from unrefined petroleum contains 90.0% CH4, 8.9% C2H6, and 1.1% C3H8 at a total pressure of 307.2 kPa. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)

A gas mixture contains CO, Ar and H 2. What is the total pressure of the mixture, if the mole fraction of H2 is 0.350 and the pressure of H 2 is 0.480 atm?

A gas mixture contains each of the following gases at the indicated partial pressures: N2, 211 torr; O2, 107 torr; and He, 149 torr. What is the total pressure in torr of the mixture? What mass in grams of each gas is present in a 1.15 - L sample of this mixture at 25.0 °C? Enter your answers numerically separated by commas.

Part 1. A closed system with a volume of 2.0 L contains radon gas and liquid water, and the container is allowed to equilibrate at 27°C until the total pressure is constant. What is the partial pressure of radon if the total pressure is 780 torr and the water vapor partial pressure is 1.0 atm? Part 2. Some helium gas is added to the system, and the total pressure increases to 1.20 atm. What is the new partial pressure of radon?

A tank contains a mixture of 52.5 g oxygen gas and 65.1 g carbon dioxide gas at 27°C. The total pressure in the tank is 9.21 atm. Calculate the partial pressures of each gas in the container.

Consider the flasks in the following diagram. What are the final partial pressures of H 2 and N2 after the stopcock between the two flasks is opened? (Assume the final volume is 3.00 L.) What is the total pressure (in torr)?

Consider the three flasks in the diagram below. Assuming the connecting tubes have negligible volume, what is the partial pressure of each gas and the total pressure after all the stopcocks are opened?

A cylinder of a gas mixture used for calibration of blood gas analyzers in medical laboratories contains 5.0% CO2, 12.0% O2, and the remainder N2 at a total pressure of 146 atm. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)

Consider the apparatus below, which shows gases in two containers and one empty container.When the valves are opened and the gases are allowed to mix at constant temperature, what is the distribution of atoms in each container? Assume that the containers are of equal volume, and ignore the volume of the tubing connecting them.

The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 155 mmHg, 476 mmHg, and 669 mmHg, respectively. What is the mole fraction of nitrogen?20.90.8800.5150.4100.366

Part A: What is the mole fraction of oxygen gas in air (see table 5.3 in the textbook)? Express your answer using two significant figures. Part B: What volume (L) of air contains 10.7 g of oxygen gas at 273 K and 1.00 atm? Express your answer using two significant figures.

A 7.70-L container holds a mixture of two gases at 27 °C. The partial pressures of gas A and gas B. respectively, are 0.306 atm and 0.574 atm. If 0.250 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

Be sure to answer all parts.A mixture of gases contains 0.310 mol CH4, 0.240 mol C2H6, and 0.300 mol C3H8. The total pressure is 1.25 atm. Calculate the partial pressures of the gases. (a) CH4 (b) C2H6 (c) C3H8

A mixture of 0.164 moles of C is reacted with 0.117 moles of O2 in a sealed, 10.0 L vessel at 500 K, producing a mixture of CO and CO2. [See reaction below] The total pressure is 0.7043 atm. What is the partial pressure of CO?C(s) + 2 O2(g) → 2 CO(g) + CO2(g)

Container A holds 712 mL of ideal gas at 2.20 atm. Container B holds 124 mL of ideal gas at 4.20 atm. If the gases are allowed to mix together, what is the resulting pressure?

Enter your answer in the provided box.What mole fraction of O2 is necessary for the partial pressure of O2 to be 2.80 atm when the total pressure is 5.73 atm?

A container with total Pressure of 2.9 atm contains 3 Gases: A, B, and C. The partial pressures of Gas A is 0.357 atm and the partial pressure of Gas B is 0.620 atm. What is the partial pressure of Gas C?

A sample of experimental welding gas composed of 56 g N2, 4.6 g O2, and 2 g Ar. What is the partial pressure exerted by O2 if the total pressure is 450 kPa?

A mixture of hydrogen and neon gases, at a total pressure of 658 mm Hg, contains 0.147 grams of hydrogen and 1.59 grams of neon. What is the partial pressure of each gas in the mixture?

A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr? Hint: what is the mole fraction of each gas?a. 256 torr b. 556 torr c. 80.0 torr d. 200. torr e. 500. torr

A mixture of krypton and nitrogen gases at a total pressure of 950 mm Hg contains krypton at a partial pressure of 450 mm Hg. If the gas mixture contains 10.9 grams of krypton, how many grams of nitrogen are present?

A gas mixture with a total pressure of 760 mmHg contains each of the following gases at the indicated partial pressures: 124 mmHg CO2, 213 mmHg Ar, and 191 mmHg O2. The mixture also contains helium gas. Part AWhat is the partial pressure of the helium gas? Express your answer in millimeters of mercury.

Hellox is helium-oxygen mixture that may be used in scuba tanks for divers working at great depths. It is also used medically as a breathing treatment.A 6.25-L tank holds helium gas at a pressure of 1031 psi. A second 6.25-L tank holds oxygen at a pressure of 274.1 psi. The two gases are mixed in a 6.25-L tank. If the temperature remains the same throughout the process, what is the pressure of the gas mixture in the tank? Assume ideal gas behaviour.

A sealed glass container contains partial pressures of 0.24 atm O 2 gas and 0.46 atm H2 gas. What is the mole fraction of H 2 in the glass container?

A gas mixture, with a total pressure of 300. torr, consists of equal masses of Ne (atomic weight 20) and Ar (atomic weight 40). What is the partial pressure of Ar in torr? A. 75 torr b. 100. torr c. 150. torr d. 200. torr e. None of these choices is correct.

A 7.40-L container holds a mixture of two gases at 51°C. The partial pressures of gas A and gas B. respectively, are 0.336 atm and 0.854 atm. lf 0.220 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 21°C is 1.26 atm, what is the partial pressure of nitrogen? The vapor pressure of water at 21°C is 18.7 mm Hg.

A mixture of hydrogen and oxygen gases contains hydrogen at a partial pressure of 441 mm Hg and oxygen at a partial pressure of 486 mm Hg. What is the mole fraction of each gas in the mixture?

A gaseous mixture contains 431.0 Torr of H2(g), 328.3 Torr of N2(g), and 81.7 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases.

A solution contains 4.90 moles of water, 1.05 moles of sucrose (C12H22O11), and 1.50 moles of glucose. Sucrose and glucose are nonvolatile. What is the mole fraction of water in this solution? Assuming an ideal mixture, what is the vapor pressure of this solution at 35°C, given that the vapor pressure of pure water at 35°C is 42.2 torr?

The picture below shows two bulbs connected by a stopcock. The large bulb, with a volume of 6.00 L, contains nitric oxide at a pressure of 0.850 atm, and the small bulb, with a volume of 1.50 L, contains oxygen at a pressure of 2.50 atm. The temperature at the beginning and the end of the experiment is 22°C. After the stopcock is opened, the gases mix and react: 2NO (g) + O2 (g) → 2NO2 (g) Which gases are present at the end of the experiment? What are the partial pressures in atm of the gases? If the gas was consumed completely, put 0 for the answer.

A mixture of He, Ne, and Ar has a pressure of 29.9 atm at 28.0°C. If the partial pressure of He is 2.03 atm and that of Ar is 2.36 atm, what is the partial pressure of Ne?

Part AIf the partial pressure of nitrogen is 592 mmHg, oxygen is 160 mmHg, argon is 7 mmHg, and trace gas is 1 mmHg, what is the atmospheric pressure?Express your answer with the appropriate units.

A sample of 5.10 mL of diethylether (C2H5OC2H5; density = 0.7134 g/mL) is introduced into a 6.50 -L vessel that already contains a mixture of N2 and O2, whose partial pressures are PN2 = 0.751 atm and PO2 = 0.207 atm. The temperature is held at 35.0 °C, and the diethylether totally evaporates. Part A Calculate the partial pressure of the diethylether. Part B Calculate the total pressure in the container.

A gas mixture contains 1.23 g N2 and 0.92 g O2 in a 1.68-L container at 24°C. Calculate the mole fraction of N2. Express your answer using two significant figures. Calculate the mole fraction of O2. Express your answer using two significant figures. Calculate the partial pressure of N2. Express your answer using two significant figures. Calculate the partial pressure of O2. Express your answer using two significant figures.

What is the pressure of the gas in this mercury manometer if h = 77 mm and atmospheric pressure is 777 mmHg?

A mixture of H2(g) and Cl2(g) exerts a total pressure of 2.50 atm. If the mole fraction of H2 is 0.490, what is the partial pressure (in atm) of H2? Show your work for partial credit. PA = XAPTotal

A gas mixture contains 75 2% nitrogen and 24 krypton by mass.What is the partial pressure of krypton in the mixture if the total pressure is 846 mmHg ? Express your answer with the appropriate units.

What is the pressure in a 7.50-L flask after 0.15 mol of carbon dioxide is added to 0.33 mol of oxygen in the flask? The temperature of the mixture is 48.0°C. a. 0.592 atm b. 1.69 atm c. 0.252 atm d. 4.80 atm e. 3.96 atm

A gas mixture with a total pressure of 700 mmHg contains each of the following gases at the indicated partial pressure: 126 mmHg CO2, 220 mmHg Ar and 188 mmHg O2. The mixture also contain helium gas.Part AWhat is the partial pressure of the helium gas?Express your answer in millimeters of mercury.

In a container containing CO, H2, and O2, what is the mole fraction of CO if the H 2 mole fraction is 0.22 and the O2 mole fraction is 0.58?

Container A holds 767 mL of ideal gas at 2 30 atm. Container B holds 129 mL of ideal gas at 4.20 atm, If the gases are allowed to mix together, what is the partial pressure of each gas in total volume?

A mixture of 0.220 moles Co, 0.350 moles H 2 and 0.640 moles He has a total pressure of 2.95 atm. What is the pressure of H2?

What is the mole fraction of O2 in a mixture of 15.1 g of O2, 8.18 g of N2, and 2.47 g of H2?

The drawing below represents a mixture of three different gases.Rank the three components in order of decreasing partial pressure.

A gas mixture contains 75.2% nitrogen and 24.8% krypton by mass.What is the partial pressure of krypton in the mixture if the total pressure is 776 mm Hg ?

Assume that an exhaled breath of air consists of 74.7 % N2, 15.4 % O2, 3.8 % CO2, and 6.1 % water vapor.If the total pressure of the gases is 0.990 atm , calculate the partial pressure of CO2.

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