Partial Pressure

Key Questions

• Question #c7420

  Dalton's Law of Partial Pressure states that the total pressure in a container will be the sum of the individual pressures of the gases present in a container.

  #P_t# = #P_1# + #P_2# + #P_3# + etc.

  Here is a video which discusses an application of this law.
  

  Many chem classes will perform an experiment to collect a gas (Hydrogen, butane etc.) in an upside-down eudiometer which is filled with water and placed into a container of water. As the gas enters the eudiometer, water is pushed out. The pressure of the gases in the eudiometer (collected gas + water vapor) will equal the atmospheric pressure in the room as long as the water level inside and outside of the eudiometer match. The pressure of the collected gas will be found by taking the room pressure and subtracting the vapor pressure of water.

  Here is a video of this lab.

  mrpauller.weebly.com · 1 · May 9 2014

• How do you do a steam distillation?
• Question #f8a34
• Can I calculate the total pressure of a mixture of gases by adding together the partial pressures of the component gases?
• What is the formula of partial pressure?
• What is the Dalton's law of partial pressures?
• Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200°C in a closed container, 1.05 atm of nitrogen gas is mixed with 2.02 atm of hydrogen gas. At equilibrium the total pressure is 2.02 atm. What is the partial pressure of hydrogen gas at equilibrium?
• What is partial pressure of oxygen in arterial blood?
• What is partial pressure gradient?
• How can I find partial pressure given moles?
• How is the partial pressure of a gas in a mixture calculated?
• How does the partial pressure of water change as the temperature increases?
• How does partial pressure affect delta G?
• How do partial pressures affect each other?
• A gas mixture contains 0.70 moles of nitrogen gas, 0.20 moles of hydrogen gas, and 0.10 moles of methane (CH4). What is the partial pressure of nitrogen?
• What are some common mistakes students make with partial pressure?
• What is an example of a partial pressure practice problem?
• What are some examples of partial pressures?
• Question #5cddc
• Question #bf6ac
• Question #bf572
• Question #e5f52
• Consider a steel container filled with 40.0 g of helium gas and 40.0 g of argon gas. What is the ratio of pressures that each gas exerts (helium:argon)? a) 1:1 b) 10:1 c) 1:10 d) 9:1
• Question #66a05
• Question #11d78
• What are the mole fraction and the mole percent of oxygen in exhaled air if P (subscript of O2) is 116 torr and a P (subscript of total) is 788 torr? I not sure if the question makes sense.
• A mixture of gases contains 319 torr N2, 273 torr O2, and 285 torr Ar. What is the total pressure of the mixture?
• A diver breathing heliox with an oxygen composition of 5.0% wants to adjust the total pressure so that #P_(O_2)= "0.21 atm"#. What must the total pressure be?
• When a container is filled with 3.00 moles of #H_2#, 2.00 moles of #O_2#, and 1.00 mole of #N_2#, the pressure in thecontainer is 768 kPa. What is the partial pressure of #O_2#?
• Question #00c38
• Question #9bc92
• Question #db8f6
• A gas mixture consists of 0.4mole of N2, 0.6 mole of O2 and 0.2 mole of argon at a total pressure of 300kPa. Calculate the partial pressure of each gas in the mixture?
• A solution contains 3.95g of CS2 and 2.43g CH3COCH3.vapor pressures at 35°C of pure CS2 and pure CH3COCH3 are 616 torr and 332 torr respectively.Assume ideal ,calculate vapor pressure of each component n the total vapor pressure?
• Question #7a92c
• A flask contains a gas mixture of methane, hydrogen. and nitrogen with partial pressures of 1 atm. 1.2 atm, and 1.1 aim, respectively. What is the total pressure of the mixture?
• Question #047bf
• Question #e7a85
• What are the partial pressures and the total pressure in a 2.50 L vessel containing the following mixture of gases at 17.8°C: 0.0274 mol #He#, 0.0431 mol #H_2#, and 0.169 mol #Ne#?
• A mixture of gases contains 0.75 mol N2, 0.30 mol O2, and 0.15 mol CO2. If the total pressure of the mixture is 1.56 atm, what is the partial pressure of each component?
• A mixture containing 2.53 g each of CH4(g), C2H4(g) and C4H10(g) is contained in a 1.50 L flask at a temperature of 25°C. How would you calculate the partial pressure of each of the gases in the mixture?
• What is the difference between the partial pressure and concentration?
• 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)?
• If you mixed three gases: 8 g of helium, 2 g of nitrogen, and 16 g of oxygen and the total pressure was 10.0 atm, what is the partial pressure of helium?
• A gas sample containing only SO2, PF3, and CO has the following mass percentage: 29.1 % SO2, 61.8 % PF3. How would you calculate the partial pressure in torr, of CO if the total pressure of sample is 684 torr?
• How would you calculate the partial pressure of CO2, given an atmospheric pressure of 760 mm Hg and a 0.04% concentration?
• Gas samples A, B, C are contained at STP. Partial pressure of sample A is 38.0 kPa and sample B is 19.0 kPa. What is the partial pressure of sample C?
• What is the partial pressure of oxygen collected over water if the temperature is 20.0°C and the total gas pressure is 735 mmHg?
• Question #c8a2e
• A 7.35-L container holds a mixture of two gases at 17 °C. The partial pressures of gas A and gas B, respectively, are .415 atm and .720 atm. If .160 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?
• The hydrogen gas is collected by displacement of water at 35.0 °C at a total pressure of 748 torr. The vapor pressure of water at 35.0 °C is 42 torr. What is the partial pressure of #H_2# if 307.8 mL of gas is collected over water from this method?
• At 15°C, a 1.00 L container contains 6.41 mol #N_2# and 3.82 mol #Ar#. What is the partial pressure of each gas, and what is the total pressure inside the container?
• Question #ad366
• A sample of gas is collected over water at a temperature of 27.0°C when the barometric pressure reading is 750.0 mm Hg. What is the partial pressure of the dry gas?
• Question #d5762
• If a mixture of gases with a total pressure of 1.0 atm contains 2 mol #He#, 4 mol #Ne#, and 2 mol #O_2#, what is the partial pressure of the #He# in the mixture?
• What are the mole fractions of each component in a mixture of 15.08 g of #O_2#, 8.17 g of #N_2#, and 2.64 g of #H_2#? What is the partial pressure in atm of each component of this mix ture if it is held in a 15.50-L vessel at 15°C?
• The osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose, #C_6H_12O_6#, is isotonic (same osmotic pressure) with blood?
• Question #ecc4f
• If oxygen is removed from a sample of air as iron rusts, what happens to the partial pressure of oxygen in the air?
• If the total atmospheric pressure of a planet was 890 mmHg and the gases in the atmosphere were 10% oxygen, 80% nitrogen, 9.5% carbon dioxide, and .5% other gases, what is the partial pressure of each gas?
• A breathing mixture used by deep-sea divers contains helium, oxygen, and carbon dioxide What is the partial pressure of oxygen at #101.4# #kPa# if #P_(He)# = #82.5# #kPa# and #P_(CO2)# = #.4# #kPa#?
• Question #748ea
• What is the vapor in oxygen gas collected by water displacement at 10°C and 75 mm Hg?
• Question #0465f
• A flask contains three times as many moles as #H_2# as it does #O_2# gas. If hydrogen and oxygen are the only present gases, what is the total pressure flask if the partial pressure due to oxygen is #P#?
• Why can you calculate the total pressure of a mixture of gases by adding together the partial pressures of the component gases?
• Question #0d4c9
• Question #15420
• Question #48d69
• A tank contains a mixture of 54.5 g of oxygen gas and 68.9 g of carbon dioxide gas at 38°C. The total pressure in the tank is 10.00 atm. How do you calculate the partial pressure (in atm) of each gas in the mixture?
• Container A holds 737 mL of ideal gas at 2.30 atm. Container B holds 114 mL of ideal gas at 4.40 atm. lf the gases are allowed to mix together, what is the resulting pressure?
• Question #5cddd
• A mixture of oxygen, hydrogen, and nitrogen exerts a total pressure of 378 kPa. If the partial pressures of oxygen and hydrogen are 212 kPa and 101 kPa respectively, what is the partial pressure exerted by nitrogen?
• A 1.50 liter flask at a temperature of 25°C contains a mixture of .158 moles of methane, .09 moles of ethane, and .044 moles of butane. What is the total pressure of the mixture inside the flask?
• A mixture of four gases exerts a total pressure of 860 mmHg. Gases A and B each exert 220 mmHg. Gas C exerts 110 mmHg. What pressure is exerted by gas D?
• Question #c446e
• A sample of argon gas is collected over water at 30.0 degrees C. The level of the water is adjusted until the total pressure in the flask is 771 torr and the volume is 250.0 mL. The vapor pressure of water is 31.8 torr at 30.0 degrees C.?
• A sample of gas is collected over water at a temperature of 35.0°C when the barometric pressure reading is 742.0 torr. What is the partial pressure of the dry gas?
• Question #7157d
• How does the partial pressure, exerted by a single component in a gaseous mixture, relate to the total pressure?
• A gas mixture has 2 atm #He#, 4.8 atm #Xe#, and 1.9 atm #O_2#. Which gas takes up the most volume in a total of 456 mL?
• A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.2 g of #O_2#, and 32.6 g of #He#. What is the partial pressure of each gas and the total pressure if the temperature of the gas is 19°C?
• A sample of nitrogen gas is collected over water at 20°C. The vapor pressure of water at 20°C is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure is 765 mmHg?
• A flask contains methane, chlorine, and carbon monoxide gases. The partial pressures of each are 0.215 atm, 50 torr, and 0.826 respectively. What is the total pressure in the flask?
• A sample of chlorine gas is collected by water displacement at 23°C. If the atmospheric pressure is 751 torr, what is the partial pressure of the chlorine?
• How do I determine entropy change between two states if given the two temperatures and the two pressures?
• Question #777e2
• Question #8b160
• What is the total pressure exerted by a mass of #2.27*g# of oxygen gas, and a mass of #0.636*g# of helium gas, if the container had a volume of #6.26*L#, and the gases were at a temperature of #51# #""^@C#?
• Question #651b6
• Question #655b9
• The degree of dissociation of #"Ca"("NO"_3)_2# in a dilute aqueous solution containing 14g of the salt per 200 g of water at #100^@"C"# is 70% .If the vapour pressure of water is 760 mmHg , what will be the vapour pressure of the solution ?
• The attached plot shows the ratio of PV to RT for 1.0 mole of nitrogen gas as a function of pressure at T=1000K. Explain why the ratio should be 1.0 for an ideal gas, and why nitrogen does not behave ideally at high pressures?
• Partial Pressure Problem?
• What is the partial pressure of #CO_2#?
• What is partial pressure and how is it used?
• How does partial pressure work?
• How would you explain partial pressure?
• What is the partial pressure of gases?
• What is the partial pressure of oxygen?
• What is meant by partial pressure of oxygen?
• How can you calculate partial pressure?
• How can you calculate the partial pressure of a gas in a mixture?
• How can you find partial pressure?
• How do partial pressures of gases influence one another?
• How do you calculate the partial pressure of hydrogen gas?
• How do you calculate the partial pressure of water?
• How does partial pressure affect the movement of oxygen?
• How can partial pressure change?
• Does partial pressure change with altitude?
• How is partial pressure related to mole fraction?
• What is partial pressure in chemistry?
• What is the partial pressure of carbon dioxide?
• What is partial pressure of oxygen at sea level?
• What is partial pressure of oxygen in blood?
• A vessel contains a mixture of nitrogen and oxygen. If the partial pressure of nitrogen is 20 atmospheres and the partial pressure of oxygen is 42.8 atmospheres, what is the total pressure inside the vessel?
• A 1.2-liter tank at a temperature of 27°C contains a mixture of 1.5 moles of oxygen, 1.2 moles of nitrogen, and 1.6 moles of hydrogen. What is the total pressure of the mixture inside the tank?
• A mixture of gases with a pressure of 800.0 Hg contains 60% nitrogen and 40% oxygen by volume. What is the partial pressure of oxygen in this mixture?
• A tank contains #N_2# at 1.0 atm and #O_2# at 2.0 atm. Helium is added to this tank until the total pressure is 6.0 atm. What is the partial pressure of the helium?
• What is the partial pressure of helium gas in a sealed vessel that has a total pressure of 205 kPa and partial pressures of 15 kPa for chlorine and 89 kPa for fluorine?
• The composition of dry air is approximately 78% nitrogen, 21% oxygen, and 1% other gases. What is the partial pressure of nitrogen at standard atmospheric pressure?
• A mixture of two gases has a total pressure of 5.7 atm. If one gas has a partial pressure of 4.1 atm, what is the partial pressure of the other gas?
• What causes the pressure inside oxygen tanks to change as they are filled?
• What is Dalton law of partial pressure?
• What is the equation for Dalton's law of partial pressure?
• What are some examples of Dalton's law of partial pressure?
• What are some example problems of Dalton's law of partial pressure?
• How would you define Dalton's law of partial pressures and relate it to atmospheric gases?
• How did Dalton come up with the law of partial pressure?
• How does Dalton's law of partial pressure work?
• How does Dalton's law of partial pressures apply to vapor pressure?
• Is Dalton's law of partial pressure dependent upon ideal behavior?
• What does Dalton's law of partial pressure mean?
• What is the Dalton law of partial pressure equation?
• What is Dalton's law of partial pressure formula?
• Why is Dalton's law of partial pressure important?
• Why is Dalton's law of partial pressure necessary?
• Question #1cee1
• Question #3d1a8
• A mixture of two gases has a total pressure of 6.7 atm. If one gas has a partial pressure of 4.1 atm, what is the partial pressure of the other gas?
• A 2.0 liter balloon at a temperature of 25°C contains 0.1 mol of oxygen and 0.4 mol of nitrogen, what is the partial pressure of nitrogen?
• How do you calculate the partial pressures of this problem?
• The composition of earths dry atmosphere is #78.8% N_2#, #21.0% O_2#, and #1.00% Ar#. Using the atospheric pressure recorded, which was 763 mm Hg with and an ambient temperature of 25 C, how do you calculate the partial pressures of these three gases?
• Assuming that the total pressure of the gases is 1.68 and that their mole ratio is 94 : 4.0 : 1.5 : 0.50, how do you calculate the partial pressure (in atmospheres) of each gas?
• A gaseous mixture of propylene and methylene fluoride, occupies a volume of 2.40L at 29°C. The partial pressure of #C_3H_6# is 0.130 atm and that of CH2F2 is 0.460 atm. How many moles of #C_3H_6# are in the sample? What is the total mass of the sample?
• How do you calculate the partial pressure of ammonia in the container after the reaction has reached completion? How do you calculate the volume of the container after the reaction has reached completion?
• A mixture of 1.24 g H2 and 1.51 g He is placed in a 1.00 L container at 28°C. How do you calculate the partial pressure of each gas and the total pressure?
• The mass percent of a three component gas sample is 11.0% #BF_3#, 74.5% #CO# and 14.5% #PF_3#. How do you calculate the partial pressure (torr) of #BF_3# if the total pressure of the sample is 0.480 atm?
• Mixture containing .538mol #He# gas, .315mol #Ne# gas .103 #Ar# gas, is confined in 7.00-L vessel at #25^o#Celsius. How do you calculate partial pressure of each gas in mixture? How would you calculate the total pressure of the mixture?
• How do you use Dalton's law to calculate partial pressure?
• A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 52.0 g of O2 and 32.1 g of He. How would you calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 17 degrees C?
• How do you find the partial pressure of oxygen?
• How would you explain the partial pressure of oxygen?
• How does partial pressure of oxygen change with altitude?
• How does the partial pressure of oxygen affect hemoglobin?
• How is partial pressure of oxygen measured?
• How do you calculate the partial pressure of oxygen in the air?
• What is the partial pressure of oxygen in air?
• What does partial pressure of oxygen mean?
• What partial pressure of oxygen is toxic?
• Why is the partial pressure of oxygen low in tissue cells?
• Why is partial pressure of oxygen lower at high altitudes?
• A mixture of #H_2# and water vapor is present in a closed vessel at 20°C. The total pressure of the system is 755.0 mmHg. Partial pressure of water vapor at 20°C equals 17.5 mmHg. What is the partial pressure of #H_2#?
• A mixture of helium and neon gases is collected over water at 28.0°C and 745 mmHg. If the partial pressure of helium is 368 mmHg, what is the partial pressure of neon?
• If a gaseous mixture is made by combining 3.54 g of Ar and 2.59 g of Kr in an evacuated 2.50 L container at 25 degrees C, what are the partial pressures of each gas and what is the total pressure by the gaseous mixture?
• A tank contains helium gas at 490 mm Hg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm?
• A sample containing 4.80 g of #O_2# gas has a volume of 15.0 L at constant pressure and temperature. What is the new volume, in liters, after 0.500 mole of #O_2# gas is added to the initial sample of 4.80 g of #O_2#?
• A flask contains oxygen, carbon dioxide, and nitrogen gases. The partial pressures of each are 11.4 atm, 5.6 atm, and 8.7 atm respectively. What is the total pressure in the flask in atm?
• Question #e9de5
• What quantity of water results from the combustion of a #0.5*g# mass of dihydrogen gas?
• Question #226ac
• What happens to the partial pressure of oxygen in a sample of air if the temperature is increased?
• If 5.0 of nitrogen gas and 5.0 g of chlorine gas are injected in to a 2.0 L vessel at a temperature of 65#"^o#C, what will the partial pressure of each gas be? What will the total pressure in the container be?
• What are the partial pressures exerted by each component exerted by a 4:1 mixture of oxygen and argon with respect to moles if the total pressure is #1*atm#?
• A certain gas mixture is held at #395^@ "C"# has the following initial partial pressures: #P_(Cl_2) = 351.4#, #P_(CO) = 342.0#, #P_(COCl_2) = 0#, all in #"torr"#. Find #K_P^@#?
• Question #b4dc0
• Question #70d16
• Question #33096
• Question #c3e2b
• How do you calculate the partial pressure of oxygen, O2, in whose composition as weight percentage is given as: CO2 = 0.04%, O2 = 22.83, N2 = 75.33% and H2O = 1.8%, f the pressure of air is given as 760 mm Hg?
• A mixture of 1.00 g #H_2# and 1.00 g #He# is placed in a 1.00-L container at 27°C. What is the partial pressure of each gas and the total pressure?
• What are the partial pressures of the gases?
• Why does oxygen occur as #O_2#, and nitrogen as #N_2#?
• An air sample contains 0.038% #CO_2#. If the total pressure is 758 mm Hg, what is the partial pressure of #CO_2#?
• Why does the boiling point of a liquid REDUCE, as the pressure of the gas above it is reduced?
• A gas mixture is made by combining 7.0 g each of Ar, Ne, and an unknown diatomic gas. At STP, the mixture occupies a volume of 16.60 L. What is the molar mass of the unknown gas?
• A gaseous mixture contains 440.0 Torr of H2(g), 365.7 Torr of N2(g), and 88.7 Torr of Ar(g). Calculate the mole fraction, X, of each of these gases?
• What is the total pressure if an anaesthetic gas is delivered at #330*mm*Hg# pressure?
• A solution, that we may consider to be ideal, is composed of a #100*g# masses EACH of ethanol and methanol....what is the vapour pressure of the solution?
• A container of gas with a pressure of 450 kPa contains three different gasses -hydrogen, oxygen, and nitrogen. If the partial pressure of the hydrogen is 210 kPa and the partial pressure of the oxygen is 125 kPa, what is the partial pressure of nitrogen?
• A vessel collects Gas B over water at 35 C. Within the container, the total pressure is 110 kPa. How do you calculate the partial pressure of Gas B if the water vapor pressure at 35°C is 5.6 kPa?
• A flask contains helium at #752*"Torr"#, and a second flask contains argon at #712*"Torr"#. What are the partial pressures of each gas in each flask?
• 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?
• If atmospheric pressure on a certain day is 749 mmHg, what is the partial pressure of nitrogen, given that nitrogen is about 78% of the atmosphere?
• A cylinder is filled with 200 moles of nitrogen, 300 moles of argon, and 5.00 moles of helium. If the gas mixture is at STP, what is the partial pressure of the argon?
• A 10.0 L flask contains 1.031 g O2 and 0.572 g CO2 at 18C. What are the partial pressures of oxygen and carbon dioxide?
• Question #2beda
• In a gaseous mixture, how does #P_"Total"# relate to the individual partial pressures, i.e. #P_1#, #P_2#...#P_n# exerted by each gaseous component?
• Abreathing mixture used by deep sea divers contains helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen at 1 atmosphere if P He- 609.5 mm Hg and P #CO_2# = 0.5 mm Hg?
• Question #05614
• Under SATP (not STP), magnesium was reacted with acid and 500 ml of hydrogen gas was collected over water. a) what is the vapour pressure of water? b) what is the pressure of the hydrogen gas? c) what amount of hydrogen was produced?
• Question #badf7
• 9. Suppose two gases in a container have a total pressure of 1.20 atm. What is the pressure of gas B if the partial pressure of gas A is 0.75 atm?
• Question #500f0
• How is the partial pressure of a component gas proportional to the percentage composition (by molar quantity) to the gaseous mixture?
• Question #32207
• A sample of nitrogen is collected over water at 20°C. The vapor pressure of water at 20°C is 18 mmHg. What is the partial pressure of the nitrogen if the total pressure is 21 mmHg?
• What is the initial partial pressure, in mmHg, of N2O5(g)?
• My textbook says that that for a mixture of #15.2*g# helium gas, and #30.6*g# dioxygen gas, the partial pressure is dominated by the helium. Can you find #P_"He"#, and #P_"dioxygen"# and #P_"Total"#?
• Question #d2ce6
• Question #d1755
• If at #"71226 Pa"# of pressure, ethoxyethane boils at #25^@ "C"#, then what vapor pressure is needed to boil at #78^@ "C"# if across the temperature range we can assume that #DeltaH_"vap" = "29.1 kJ/mol"#?
• At equilibrium, the partial pressure of #SO_2# is 35.0 atm and that of #O_2# is 15.9 atm. What is the partial pressure of #SO_3# in atm?
• What is the partial pressure of water vapor in oxygen gas collected by water displacement at 10°C and 750 mm Hg?
• If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, what is the partial pressure of oxygen on Everest?
• The total pressure is 600 mmHg after 0.50 moles of nitrogen gas, #N_2#, and 1.0 mole of nitrogen dioxide, #NO_2#, gas are mixed in a closed container. There is no reaction between the gases. What is the partial pressure of the nitrogen dioxide?
• A container holds 6.4 moles of gas. Hydrogen gas makes up 25% of the total moles in the container if the total pressure is 1.24 atm. What is the partial pressure of hydrogen?
• A gaseous mixture of helium and neon at #1*atm# contains a partial pressure of #0.60*atm# with respect to helium. What is #P_"Ne"#?
• A solution of liquid toluene dissolved in liquid benzene has a benzene mole fraction of .850. Calculate the vapor pressure of the solution given that the vapor pressures of pure benzene and toulene are 183 mmHg and 59.2 mmHg, respectively?
• Question #aae8e
• The molar quantities of THREE GASES sum to #1.02*mol#. What pressure would result if the gases were heated to #301*K#, and confined to a #30*L# volume?
• The pressure of gases inside a rigid container is #"99000 kPa"#. The composition of the gases is #68%# nitrogen gas, #23%# oxygen gas, and #9%# neon gas. What is the partial pressure of each gas?
• Question #da319
• Question #cce86
• Question #c5cb2
• A gaseous mixture at #780*mm*Hg# pressure contains carbon dioxide, and dioxygen. If #P_(CO_2)=560*mm*Hg#, what is #P_(O_2)#?
• Question #28dda
• A tank of gas has partial pressures of nitrogen and oxygen equal to #1.61 xx 10^4# #"kPa"# and #4.34 xx 10^5# #"kPa"#, respectively. What is the total pressure of the tank?
• A tank contains a mixture of helium, neon, and argon gases. lf the total pressure in the tank is 490. mmHg and the partial pressures of helium and argon are 21.5 mmHg and 10.2 mmHg, respectively, what is the partial pressure of neon?
• A mixture of 0.2 mole O2 and 0.4 mole N2 gas is enclosed in a vessel of certain volume at 27C and 800 torr. If volume of mixture is doubled at same temperature then determine pressure of mixture and individual gases?
• A sample of nitrogen gas was collected via water displacement. Therefore, the sample is saturated with water vapor. If the total pressure of the mixture at 21 °C is 1.50 atm, what is the partial pressure of nitrogen?
• In a gaseous mixture of a #2.0*L# volume, at #755*"mm Hg"#, and a temperature of #346*K#, #P_"dinitrogen"=355*mm*Hg#. What are the molar quantities of helium and dinitrogen?
• It was found that in a diving gas mixture for a certain altitude, the total predicted pressure is #"8.38 atm"#. If the partial pressure of oxygen gas must be #"0.21 atm"# underwater, what must the mol fraction be of oxygen gas?
• Question #38bc1
• Suppose #"6g"# of #"H"_2# and #"16 g"# of #"CH"_4# are in a #"1-L"# box divided in half by a thin partition, each gas at the same initial pressure #P# in #"atm"#. Upon mixing the gases, find the total pressure?
• The composition of dry air is approximately 78% nitrogen, 21% oxygen, and 1% other gases. What is the partial pressure of nitrogen at standard atmospheric pressure (101.3 kPa)?
• Which of the following binary solutions of volatile liquids have negative deviation?
• A sample of hydrogen gas is collected over water at 25°C. The total pressure of the hydrogen and water vapor is 116.0 kPa. The partial pressure of water vapor at this temperature is 3.2 kPa. What is the pressure of the hydrogen gas alone?
• A container under #2558*"psi"# pressure contains carbon dioxide and whose partial pressure is #54.6*"bar"# and #NO_2#? What is #P_(NO_2)# in atmospheres?
• Question #83193
• Question #60dd4
• If equal mols of #"N"_2# and #"Ar"# are in the same container with a total pressure of #"10 atm"#, #(A)# what are their partial pressures? #(B)# what is the effusion speed of #"H"_2# if that of #"He"# is #"600 m/s"# at a certain temperature?
• At a total pressure of #"1 atm"#, if the mol percentages of #"CO"_2#, #"O"_2#, and #"N"_2# are #5%#, #15%#, and #80%# respectively, what are the partial pressures?
• A gas cylinder contains 2.0 mol of gas X and 6.0 mol of gas Y at a total pressure of 2.1 atm. What is is partial pressure of gas Y?
• Question #c0267
• Question #a2b19
• Equal masses of methane and hydrogen are mixed in an empty container. At 25 degree Celsius. The fraction of total pressure exerted by hydrogen will be?
• When #"4 g H"_2# and #"32 g O"_2# are mixed, what is the partial pressure of oxygen at a total pressure of #P#?
• What is the partial pressure of the helium gas? Express your answer in millimeters of mercury.
• A mixture of .250 moles O2, .297 moles N2, and .134 moles Ar has a total pressure of 1.95 atm. What is the mole fraction of O2 and what is the partial pressure of O2?
• A mixture of #"N"_2#, #"O"_2#, and #"Ar"# has mole fractions of #"N"_2 = .780#, #"O"_2 = .210#, and #"Ar" = .010#. What is the partial pressure of #"O"_2# if the total pressure of the mixture is #"750 torr"#?
• Question #b786d
• A scuba diver is at a depth of 355 m, where the pressure is 36.5 atm. What should be the mole fraction of #O_2# in the gas mixture the diver breathes in order to have the same partial pressure of oxygen in his lungs as he would at sea level?
• A mixture of 0.166 mols of #"C"# reacted with 0.117 mols of #"O"_2# in a sealed, 10.0 L vessel at 500.0 K, producing a mixture of #"CO"# and #"CO"_2#. The reaction is: #3"C"(s)+2"O"_2​(g)-> 2"CO"(g)+"CO"_2​(g)#. What is the partial pressure of #"CO"#?
• Find the partial pressure in a solution containing ethanol and 1-propanol with a total vapor pressure of #"56.3 torr"#? The pure vapor pressures are #"100.0 torr"# and #"37.6 torr"#, respectively, and the solution has a mol fraction of #0.300# of ethanol.
• Can someone help me please? thanks!
• What is the solubility of ammonia at #0# #""^@C#, and #60# #""^@C#?
• Why some gases are collected over the water?? Reasons please
• Question #cc3ae
• Calculate the mole fraction of methanol in the vapor phase at #63.5°C# for an ideal solution containing #25.0g# of pure methanol and #75.0g# of pure ethanol?
• Question #af457
• Question #a5ed9
• Question #a37c4
• Question #956b2
• Determine the total pressure of a gas mixture that contains oxygen, nitrogen, and helium if the partial pressures of the gases are as follows: #"P"_ ("O"_ 2) = "20.0 kPa"#, #P_ ("N"_ 2) = "46.7 kPa"#, and #P_ "He" = "26.7 kPa"# ?
• A mixture of #"N"_2#, #"O"_2#. and #"CO"_2# has a total pressure of #"740 torr"# In this mixture, the partial pressure of #"N"_2# is #"120 torr"# and the partial pressure of #"O"_2# is #"400 torr"#. What is the partial pressure of #"CO"_2# ?
• A 0.2 mol sample of N2 , CO2 with a pressure of 840 torr is exposed to solid CaO which react with theCO2 to form solidCaCO3 assume the reaction goes to completion complete pressure the gas had dropped to 320 how many moles of CO2 in origin mixtur? how
• A mixture of #2.00# moles of #"H"_2#, #3.00# moles of #"NH"_3#, #4.00# moles of #"CO"_2#, and #5.00# moles of #"N"_2# exerts a total pressure of #"800. mmHg"#. What is the partial pressure of each gas?
• What is the partial pressure of #"O"_2# in air at #"1 atm"# given that #21%# of air molecules are #"O"_2# ?
• What is the partial pressure of #"CO"_2# in a container that holds 5 moles of #"CO"_2#, 3 moles of #"N"_2#, and 1 mole #"H"_2# and has a total pressure of 1.05 atm?
• Starting with #\tt{SO_3(g)}# at #\sf{"1.00 atm"}#, what will be the total pressure when equilibrium is reached with the following reaction at #\sf{"700 K"}#?
• For the following reaction, with #\sf{K_p=28.5" @ 25°C"}#; if #\tt{KO_2}# solid and #\tt{CO_2(g)}# are placed in an evacuated flask and equilibrium is established, what is #\tt{P_(O_2)}# at equilibrium...?