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1 Million+ Step-by-step solutionsmath books Q:Gaseous iodine pentafluoride, IF5, can be prepared by the reactionGaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine:
I2 (s) + 5F2 (g) → 2IF5 (g)
A 5.00-L flask containing 10.0 g I2 is charged with 10.0 g F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125oC.
(a) What is the partial pressure of IF5 in the flask?
(b) What is the mole fraction of IF5 in the flask?
(c) Draw the Lewis structure of IF5.
(d) What is the total mass of reactants and products in the flask?
Q:How does a gas compare with a liquid for eachHow does a gas compare with a liquid for each of the following properties?
(a) Density,
(b) Compressibility,
(c) Ability to mix with other substances of the same phase to form homogeneous mixtures,
(d) Ability to conform to the shape of its container.
Q:A 6.53-g sample of a mixture of magnesium carbonate andA 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces 1.72 L of carbon dioxide gas 28oC at and 743 torr pressure.
(a) Write balanced chemical equations for the reactions that occur between hydrochloric acid and each component of the mixture.
(b) Calculate the total number of moles of carbon dioxide that forms from these reactions.
(c) Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture.
Q:(a) A liquid and a gas are moved to larger(a) A liquid and a gas are moved to larger containers. How does their behavior differ once they are in the larger containers? Explain the difference in molecular terms.
(b) Although liquid water and carbon tetrachloride, CCl4 (l), do not mix, their vapors form a homogeneous mixture. Explain.
(c) Gas densities are generally reported in grams per liter, whereas liquid densities are reported in grams per milliliter. Explain the molecular basis for this difference.
Q:Suppose that a woman weighing 130 lb and wearing high-heeledSuppose that a woman weighing 130 lb and wearing high-heeled shoes momentarily places all her weight on the heel of one foot. If the area of the heel is 0.50 in2 calculate the pressure exerted on the underlying surface in
(a) Kilopascals,
(b) Atmospheres,
(c) Pounds per square inch.
Q:A set of bookshelves rests on a hard floor surfaceA set of bookshelves rests on a hard floor surface on four legs, each having a cross-sectional dimension of 3.0 x 4.1 cm in contact with the floor. The total mass of the shelves plus the books stacked on them is 262 kg. Calculate the pressure in pascals exerted by the shelf footings on the surface.
Q:(a) How high in meters must a column of water(a) How high in meters must a column of water be to exert a pressure equal to that of a 760-mm column of mercury? The density of water is 1.0 g/ml, whereas that of mercury is
13.6 g / mL.
(b) What is the pressure, in atmospheres, on the body of a diver if he is 39 ft below the surface of the water when atmospheric pressure at the surface is 0.97 atm?
Q:The compound 1-iodododecane is a nonvolatile liquid with a densityThe compound 1-iodododecane is a nonvolatile liquid with a density of 1.20 g/mL. The density of mercury is 13.6 g/mL. What do you predict for the height of a barometer column based on 1-iodododecane, when the atmospheric pressure is 749 torr?
Q:Each of the following statements concerns a mercury barometer suchEach of the following statements concerns a mercury barometer such as that shown in Figure 10.2. Identify any incorrect statements and correct them.
(a) The tube must be 1cm2 in cross-sectional area.
(b) At equilibrium the force of gravity per unit area acting on the mercury column equals the force of gravity per unit area acting on the atmosphere.
(c) The column of mercury is held up by the vacuum at the top of the column.
(d) If you took the mercury barometer with you on a trip from the beach to high mountains, the height of the mercury column would increase with elevation.
Each of the following statements concerns a mercury barometer suchQ:You have a sample of gas in a container withYou have a sample of gas in a container with a movable piston, such as the one in the drawing.
(a) Redraw the container to show what it might look like if the temperature of the gas is increased from 300 K to 500 K while the pressure is kept constant.
(b) Redraw the container to show what it might look like if the external pressure on the piston is increased from 1.0 atm. to 2.0 atm. while the temperature is kept constant.
(c) Redraw the container to show what it might look like if the temperature of the gas decreases from 300 K to 200 K while the pressure is kept constant (assume the gas does not liquefy).
You have a sample of gas in a container withQ:Suppose you make a mercury barometer using a glass tubeSuppose you make a mercury barometer using a glass tube about 50 cm in length, closed at one end. What would you expect to see if the tube is filled with mercury and inverted in a mercury dish, as in Figure 10.2? Explain.
Suppose you make a mercury barometer using a glass tubeQ:Perform the following conversions: (a) 0.912 atm to torr, (b) 0.685 barPerform the following conversions:
(a) 0.912 atm to torr,
(b) 0.685 bar to kilopascals,
(c) 655 mm Hg to atmospheres,
(d) 1.323 x 105 Pa to atmospheres,
(e) 2.50 atm to psi.
Q:Perform the following conversions: (a) 0.912 atm to torr, (b) 0.685Perform the following conversions:
(a) 0.912 atm to torr,
(b) 0.685 bar to kilopascals,
(c) 655 mm Hg to atmospheres,
(d) 1.323 x 105 to atmospheres,
(e) 2.50 atm to psi.
Q:In the United States, barometric pressures are generally reported inIn the United States, barometric pressures are generally reported in inches of mercury (in. Hg) on a beautiful summer day in Chicago the barometric pressure is 30.45 in. Hg.
(a) Convert this pressure to torr.
(b) Convert this pressure to atm.
(c) A meteorologist explains the nice weather by referring to a “high-pressure area.” In light of your answer to parts (a) and (b), explain why this term makes sense.
Q:Hurricane Wilma of 2005 is the most intense hurricane onHurricane Wilma of 2005 is the most intense hurricane on record in the Atlantic basin, with a low-pressure reading of 882 mbar (milli bars). Convert this reading into
(a) Atmospheres,
(b) Torr,
(c) Inches of Hg.
Q:If the atmospheric pressure is 0.995 atm, what is theIf the atmospheric pressure is 0.995 atm, what is the pressure of the enclosed gas in each of the three cases depicted in the drawing? Assume that the gray liquid is mercury.
If the atmospheric pressure is 0.995 atm, what is theQ:An open-end manometer containing mercury is connected to a containerAn open-end manometer containing mercury is connected to a container of gas, as depicted in Sample Exercise 10.2. What is the pressure of the enclosed gas in torr in each of the following situations?
(a) The mercury in the arm attached to the gas is 15.4 mm higher than in the one open to the atmosphere; atmospheric pressure is 0.985 atm.
(b) The mercury in the arm attached to the gas is 12.3 mm lower than in the one open to the atmosphere; atmospheric pressure is 0.99 atm.
Q:You have a gas confined to a cylinder with aYou have a gas confined to a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if you do the following?
(a) Decrease the volume to one-fourth the original volume while holding the temperature constant.
(b) Reduce the temperature (in kelvins) to half its original value while holding the volume constant.
(c) Reduce the amount of gas to one-fourth while keeping the volume and temperature constant.
Q:A fixed quantity of gas at 21oC exhibits a pressureA fixed quantity of gas at 21oC exhibits a pressure of 752 torr and occupies a volume of 5.12 L.
(a) Calculate the volume the gas will occupy if the pressure is increased to 1.88 atm while the temperature is held constant.
(b) Calculate the volume the gas will occupy if the temperature is increased to 175oC while the pressure is held constant.
Q:(a) How is the law of combining volumes explained by(a) How is the law of combining volumes explained by Avogadro’s hypothesis?
(b) Consider a 1.0-L flask containing neon gas and a 1.5-L flask containing xenon gas. Both gases are at the same pressure and temperature. According to Avogadro’s law, what can be said about the ratio of the number of atoms in the two flasks?
(c) Will 1 mol of an ideal gas always occupy the same volume at a given temperature and pressure? Explain.
Q:Consider the sample of gas depicted here. What would theConsider the sample of gas depicted here. What would the drawing look like if the volume and temperature remained constant while you removed enough of the gas to decrease the pressure by a factor of 2?
Consider the sample of gas depicted here. What would theQ:Nitrogen and hydrogen gases react to form ammonia gas asNitrogen and hydrogen gases react to form ammonia gas as follows:
N2 (g) + 3 H2 → 2NH3 (g)
At a certain temperature and pressure, 1.2 L of N2 reacts with 3.6 L of H2. If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure, will be produced?
Q:(a) What is an ideal gas? (b) Show how Boyle’s law,(a) What is an ideal gas?
(b) Show how Boyle’s law, Charles’s law, and Avogadro’s law can be combined to give the ideal-gas equation.
(c) Write the ideal-gas equation, and give the units used for each term when R = 0.08206 L-atm / mol-K.
(d) If you measure pressure in bars instead of atmospheres, calculate the corresponding value of R in L-bar / mol-K.
Q:(a) What conditions are represented by the abbreviation STP? (b) What(a) What conditions are represented by the abbreviation STP?
(b) What is the molar volume of an ideal gas at STP?
(c) Room temperature is often assumed to be 25oC Calculate the molar volume of an ideal gas at 25oC and 1 atm pressure.
Q:Suppose you are given two 1-L flasks and told thatSuppose you are given two 1-L flasks and told that one contains a gas of molar mass 30, the other a gas of molar mass 60, both at the same temperature. The pressure in flask A is X atm, and the mass of gas in the flask is 1.2 g. The pressure in flask B is 0.5 X atm, and the mass of gas in that flask is 1.2 g. Which flask contains the gas of molar mass 30, and which contains the gas of molar mass 60?
Q:Suppose you are given two flasks at the same temperature,Suppose you are given two flasks at the same temperature, one of volume 2 L and the other of volume 3 L. The 2-L flask contains 4.8 g of gas, and the gas pressure is X atm. The 3-L flask contains 0.36 g of gas, and the gas pressure is 0.1X. Do the two gases have the same molar mass? If not, which contains the gas of higher molar mass?
Q:Complete the following table for an ideal gas:Complete the following table for an ideal gas:
Complete the following table for an ideal gas:Q:Calculate each of the following quantities for an ideal gas: (a)Calculate each of the following quantities for an ideal gas:
(a) The volume of the gas, in liters, if 1.50mol has a pressure of 1.25 atm at a temperature of -6 °C;
(b) The absolute tempera ture of the gas at which 3.33 x 10-3occupies 478 mL at 750 torr;
(c) The pressure, in atmospheres, if 0.00245mol occupies 413 mL at 138oC;
(d) The quantity of gas, in moles, if 126.5 L at 54oC has a pressure of 11.25 kPa.
Q:The Goodyear blimps, which frequently fly over sporting events, holdThe Goodyear blimps, which frequently fly over sporting events, hold approximately 175000ft3 of helium. If the gas is at 23oC and 1.0 atm, what mass of helium is in a blimp?
Q:A neon sign is made of glass tubing who’s insideA neon sign is made of glass tubing who’s inside diameter is 2.5 cm and whose length is 5.5 m. If the sign contains neon at a pressure of 1.78 torr at 35oC, how many grams of neon are in the sign? (The volume of a cylinder is πr2h.)
Q:(a) Calculate the number of molecules in a deep breath(a) Calculate the number of molecules in a deep breath of air whose volume is 2.25 L at body temperature, 37oC, and a pressure of 735 torr.
(b) The adult blue whale has a lung capacity of 5.0 x 103 L. Calculate the mass of air (assume an average molar mass 28.98 g>mol) contained in an adult blue whale’s lungs at 0.0°C and 1.00 atm, assuming the air behaves ideally.
Q:Imagine that the reaction 2CO (g) + O2 (g) →Imagine that the reaction
2CO (g) + O2 (g) → 2CO2 (g)
Occurs in a container that has a piston that moves to maintain a constant pressure when the reaction occurs at constant temperature
(a) What happens to the volume of the container as a result of the reaction? Explain.
(b) If the piston is not allowed to move, what happens to the pressure as a result of the reaction?
Q:(a) If the pressure exerted by ozone, O3, in the(a) If the pressure exerted by ozone, O3, in the stratosphere is 3.0 x 10-3 and the temperature is 250 K, how many ozone molecules are in a liter?
(b) Carbon dioxide makes up approximately 0.04% of Earth’s atmosphere. If you collect a 2.0-L sample from the atmosphere at sea level (1.00 atm) on a warm day (27 °C), how many CO2 molecules are in your sample?
Q:A scuba divers tank contains 0.29 kg of O2 compressedA scuba divers tank contains 0.29 kg of O2 compressed into a volume of 2.3 L.
(a) Calculate the gas pressure inside the tank at 9oC.
(b) What volume would this oxygen occupy at and 0.95 atm?
Q:An aerosol spray can with a volume of 250 mLAn aerosol spray can with a volume of 250 mL contain 2.30 g of propane gas (C3H8) as a propellant.
(a) If the can is at 23oC, what is the pressure in the can?
(b) What volume would the propane occupy at STP?
(c) The can’s label says that exposure to temperatures above 130oF may cause the can to burst. What is the pressure in the can at this temperature?
Q:Chlorine is widely used to purify municipal water supplies andChlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of Cl2 gas is 8.70 L at 895 torr and 24oC.
(a) How many grams of Cl2 are in the sample?
(b)What volume will the Cl2 occupy at STP?
(c) At what temperature will the volume be 15.00 L if the pressure is 8.76 x 102 torr?
(d) At what pressure will the volume equal 5.00 L if the temperature is 58oC?
Q:Many gases are shipped in high-pressure containers. Consider a steelMany gases are shipped in high-pressure containers. Consider a steel tank whose volume is 55.0 gallons that contains O2 gas at a pressure of 16,500 kPa at 23oC.
(a) What mass of O2 does the tank contain?
(b) What volume would the gas occupy at STP?
(c) At what temperature would the pressure in the tank equal 150.0 atm?
(d) What would be the pressure of the gas, in kPa, if it were transferred to a container at 24oC whose volume is 55.0 L?
Q:In an experiment reported in the scientific literature, male cockroachesIn an experiment reported in the scientific literature, male cockroaches were made to run at different speeds on a miniature treadmill while their oxygen consumption was measured. In one hour the average cockroach running at 0.08 km/hr consumed 0.8 mL of O2 at 1 atm pressure and per gram of insect mass.
(a) How many moles of O2 would be consumed in 1 hr by a 5.2-g cockroach moving at this speed?
(b) This same cockroach is caught by a child and placed in a 1-qt fruit jar with a tight lid. Assuming the same level of continuous activity as in the research, will the cockroach consume more than 20% of the available O2 in a 48-hr period? (Air is 21 mol percent O2.)
Q:The physical fitness of athletes is measured by “VO2 max,”The physical fitness of athletes is measured by “VO2 max,” which is the maximum volume of oxygen consumed by an individual during incremental exercise (for example, on a treadmill). An average male has a VO2 max of 45 mL O2/kg body mass/min, but a world-class male athlete can have a VO2 max reading of 88.0 mL O2/kg body mass/min. (a) Calculate the volume of oxygen, in mL, consumed in 1 hr by an average man who weighs 185 lbs and has a VO2 max reading of 47.5 mL O2/kg body mass/min.
(b) If this man lost 20 lb, exercised, and increased his VO2 max to 65.0 mL O2/kg body mass/min, how many mL of oxygen would he consume in 1 hr?
Q:Mercury is a liquid at room temperature and pressure, butMercury is a liquid at room temperature and pressure, but its vapor is present in the atmosphere from natural sources, such as volcanoes, and from human (“anthropogenic”) activities such as coal burning and gold mining. Elemental Hg becomes extremely toxic when oxidized to Hg (I) or Hg (II) compounds.
(a) The Environmental Protection Agency has estimated that 119 tons of mercury are currently emitted to Earth’s atmosphere annually due to human activities; this has decreased significantly from the mid-1970s before pollution controls were in place. What volume would the 119 tons of mercury occupy if it were a pure vapor at 1.00 atm and 298 K?
(b) Geological records suggest that before the Industrial Revolution began in 1750, the baseline level of atmospheric Hg was 35 ppb (parts per billion, by volume, or 35 L Hg for every 109 L of air); current estimates are 245 ppb. For an estimated atmospheric volume of 51 x 1012 m3, calculate the number of moles Hg estimated to be in the atmosphere today.
Q:After the large eruption of Mount St. Helens in 1980,After the large eruption of Mount St. Helens in 1980, gas samples from the volcano were taken by sampling the downwind gas plume. The unfiltered gas samples were passed over a gold coated wire coil to absorb mercury (Hg) present in the gas. The mercury was recovered from the coil by heating it and then analyzed. In one particular set of experiments scientists found a mercury vapor level of 1800 ng of Hg per cubic meter in the plume at a gas temperature of 10oC. Calculate
(a) The partial pressure of Hg vapor in the plume,
(b) The number of Hg atoms per cubic meter in the gas,
(c) The total mass of Hg emitted per day by the volcano if the daily plume volume was 1600km3.
Q:Which gas is most dense at 1.00 atm and 298Which gas is most dense at 1.00 atm and 298 K: CO2, N2O, or Cl2? Explain.
Q:Suppose you have a fixed amount of an ideal gasSuppose you have a fixed amount of an ideal gas at a constant volume. If the pressure of the gas is doubled while the volume is held constant, what happens to its temperature?
Q:Rank the following gases from least dense to most denseRank the following gases from least dense to most dense at atm and 298 K: SO2, HBr, CO2 Explain.
Q:Which of the following statements best explains why a closedWhich of the following statements best explains why a closed balloon filled with helium gas rises in air?
(a) Helium is a monatomic gas, whereas nearly all the molecules that make up air, such as nitrogen and oxygen, are diatomic.
(b) The average speed of helium atoms is higher than the average speed of air molecules, and the higher speed of collisions with the balloon walls propels the balloon upward.
(c) Because the helium atoms are of lower mass than the average air molecule, the helium gas is less dense than air. The mass of the balloon is thus less than the mass of the air displaced by its volume.
(d) Because helium has a lower molar mass than the average air molecule, the helium atoms are in faster motion. This means that the temperature of the helium is higher than the air temperature. Hot gases tend to rise.
Q:(a) Calculate the density of NO2 gas at 0.970 atm(a) Calculate the density of NO2 gas at 0.970 atm and 35oC.
(b) Calculate the molar mass of a gas if 2.50 g occupies 0.875 L at 685 torr and 35oC.
Q:(a) Calculate the density of sulfur hexafluoride gas at 707(a) Calculate the density of sulfur hexafluoride gas at 707 torr and 21oC.
(b) Calculate the molar mass of a vapor that has a density of 7.135 g/L at 12oC and 743 torr.
Q:In the Dumas-bulb technique for determining the molar mass ofIn the Dumas-bulb technique for determining the molar mass of an unknown liquid, you vaporize the sample of a liquid that boils below 100oC in a boiling-water bath and determine the mass of vapor required to fill the bulb. From the following data, calculate the molar mass of the unknown liquid: mass of unknown vapor, 1.012 g; volume of bulb, 354cm3; pressure, 742 torr; temperature, 99 °C.
In the Dumas-bulb technique for determining the molar mass ofQ:Magnesium can be used as a “getter” in evacuated enclosuresMagnesium can be used as a “getter” in evacuated enclosures to react with the last traces of oxygen. (The magnesium is usually heated by passing an electric current through a wire or ribbon of the metal.) If an enclosure of 0.452 L has a partial pressure of O2 of 3.5 x 10-6 torr at 27oC, what mass of magnesium will react according to the following equation?
2Mg (s) + O2 (g) → 2 MgO (s)
Q:Calcium hydride, CaH2, reacts with water to form hydrogen gas: CaH2Calcium hydride, CaH2, reacts with water to form hydrogen gas:
CaH2 (s) + 2 H2O (l) → Ca (OH)2 (aq) + 2H2 (g)
This reaction is sometimes used to inflate life rafts, weather balloons, and the like, when a simple, compact means of generating H2 is desired. How many grams of CaH2 are needed to generate 145 L of H2 gas if the pressure of H2 is 825 torr at 21 °C?
Q:The metabolic oxidation of glucose, C6H12O6, in our bodies producesThe metabolic oxidation of glucose, C6H12O6, in our bodies produces CO2, which is expelled from our lungs as a gas:
C6H12O6 (aq) + 6O2 (g) → 6CO2 (g) + 6H2O (l)
(a) Calculate the volume of dry CO2 produced at body temperature and 0.970 atm when 24.5 g of glucose is consumed in this reaction.
(b) Calculate the volume of oxygen you would need, at 1.00 atm and 298 K, to completely oxidize 50.0 g of glucose.
Q:The apparatus shown here has two gas-filled containers and oneThe apparatus shown here has two gas-filled containers and one empty container, all attached to a hollow horizontal tube. 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 connecting tube. Which gas has the greater partial pressure after the valves are opened?
The apparatus shown here has two gas-filled containers and oneQ:Both Jacques Charles and Joseph Louis Guy-Lussac were avid balloonists.Both Jacques Charles and Joseph Louis Guy-Lussac were avid balloonists. In his original flight in 1783, Jacques Charles used a balloon that contained approximately 31,150 L of H2. He generated the H2 using the reaction between iron and hydrochloric acid:
Fe (s) + 2HCl (aq) → FeCl2 (aq) + H2 (g)
How many kilograms of iron were needed to produce this volume of H2 if the temperature was 22oC?
Q:Hydrogen gas is produced when zinc reacts with sulfuric acid: Zn(s)Hydrogen gas is produced when zinc reacts with sulfuric acid:
Zn(s) + H2SO4 (aq) → ZnSO4 (aq) + H2(g)
If 159 mL of wet H2 is collected over water at 24oC and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is tabulated in Appendix B.)
Q:Acetylene gas, C2H2 (g), can be prepared by the reactionAcetylene gas, C2H2 (g), can be prepared by the reaction of calcium carbide with water:
CaC2 (s) + 2 H2O (l) → Ca (OH)2 (s) + C2H2 (g)
Calculate the volume of C2H2 that is collected over water at by reaction of 1.524 g of CaC2 if the total pressure of the gas is 753 torr. (The vapor pressure of water is tabulated in Appendix B.)
Q:Consider the apparatus shown in the following drawing. (a) WhenConsider the apparatus shown in the following drawing.
(a) When the valve between the two containers is opened and the gases allowed mixing, how does the volume occupied by the N2 gas change? What is the partial pressure of N2 after mixing?
(b) How does the volume of the O2 gas change when the gases mix? What is the partial pressure of O2 in the mixture?
(c) What is the total pressure in the container after the gases mix?
Consider the apparatus shown in the following drawing.  
(a) WhenQ:Consider a mixture of two gases, A and B, confinedConsider 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?
(a) The partial pressure of gas A,
(b) The total pressure in the vessel,
(c) The mole fraction of gas B.
Q:A mixture containing 0.765 mol He (g), 0.330 mol NeA mixture containing 0.765 mol He (g), 0.330 mol Ne (g) and 0.110 mol Ar (g) is confined in a 10.00-L vessel at 25oC.
(a) Calculate the partial pressure of each of the gases in the mixture.
(b) Calculate the total pressure of the mixture.
Q:A deep-sea diver uses a gas cylinder with a volumeA deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.2 g of O2 and 32.6 g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 19oC.
Q:The atmospheric concentration of CO2 gas is presently 390 ppmThe 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?
Q:A plasma-screen TV contains thousands of tiny cells filled withA plasma-screen TV contains thousands of tiny cells filled with a mixture of Xe, Ne, and He gases that emits light of specific wavelengths when a voltage is applied. A particular plasma cell, 0.900 mm x 0.300 mm x 10.0 mm, contains 4% Xe in a 1:1 Ne : He mixture at a total pressure of 500 torr. Calculate the number of Xe, Ne, and He atoms in the cell and state the assumptions you need to make in your calculation.
Q:A piece of dry ice (solid carbon dioxide) with aA piece of dry ice (solid carbon dioxide) with a mass of 5.50 g is placed in a 10.0-L vessel that already contains air at 705 torr and 24oC. After the carbon dioxide has totally vaporized, what is the partial pressure of carbon dioxide and the total pressure in the container at 24oC?
Q:The accompanying drawing represents a mixture of three different gases.The accompanying drawing represents a mixture of three different gases.
(a) Rank the three components in order of increasing partial pressure.
(b) If the total pressure of the mixture is 1.40 atm, calculate the partial pressure of each gas.
The accompanying drawing represents a mixture of three different gases.Q:A sample of 5.00 mL of diethylether (C2H5OC2H5, density =A sample of 5.00 mL of diethylether (C2H5OC2H5, density = 0.7134 g / mL) is introduced into a 6.00-L vessel that already contains a mixture of N2 and O2, whose partial pressures are PN2 = 0.751 atm and PO2 = 0.208 atm. The temperature is held at 35.0oC, and the diethylether totally evaporates.
(a) Calculate the partial pressure of the diethylether.
(b) Calculate the total pressure in the container.
Q:A mixture of gases contains 0.75 mol N2, 0.30 molA 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 2.15 atm, what is the partial pressure of each component?
Q:A mixture of gases contains 10.25 g of N2, 1.83A mixture of gases contains 10.25 g of N2, 1.83 g of H2, and 7.95 g of NH3. If the total pressure of the mixture is 1.85 atm, what is the partial pressure of each component?
Q:At an underwater depth of 250 ft, the pressure isAt an underwater depth of 250 ft, the pressure is 8.38 atm. What should the mole percent of oxygen be in the diving gas for the partial pressure of oxygen in the mixture to be 0.21 atm, the same as in air at 1 atm?
Q:(a) What are the mole fractions of each component in(a) What are the mole fractions of each component in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
(b) What is the partial pressure in atm of each component of this mixture if it is held in a 15.50-L vessel at 15 °C?
Q:A quantity of N2 gas originally held at 5.25 atmA quantity of N2 gas originally held at 5.25 atm pressure in a 1.00-L container at 26oC is transferred to a 12.5-L container at 20oC .A quantity of O2 gas originally at 5.25 atm and 26oC in a 5.00-L container is transferred to this same container. What is the total pressure in the new container?
Q:A sample of 3.00 g of SO2 (g) originally inA sample of 3.00 g of SO2 (g) originally in a 5.00-L vessel at 21oC is transferred to a 10.0-L vessel at 26oC. A sample of 2.35 g N2 (g) originally in a 2.50-L vessel at 20oC is transferred to this same 10.0-L vessel.
(a) What is the partial pressure of SO2 (g) in the larger container?
(b) What is the partial pressure of N2 (g) in this vessel?
(c) What is the total pressure in the vessel?
Q:Indicate which of the following statements regarding the kinetic molecularIndicate which of the following statements regarding the kinetic molecular theory of gases are correct. For those that are false, formulate a correct version of the statement.
(a) The average kinetic energy of a collection of gas molecules at a given temperature is proportional to m 1/2.
(b) The gas molecules are assumed to exert no forces on each other.
(c) All the molecules of a gas at a given temperature have the same kinetic energy.
(d) The volume of the gas molecules is negligible in comparison to the total volume in which the gas is contained.
(e) All gas molecules move with the same speed if they are at the same temperature.
Q:On a single plot, qualitatively sketch the distribution of molecularOn a single plot, qualitatively sketch the distribution of molecular speeds for
(a) Kr (g) at – 50oC,
(b) Kr (g) at – 0oC,
(c) Ar (g) at – 0oC
Q:Newton had an incorrect theory of gases in which heNewton had an incorrect theory of gases in which he assumed that all gas molecules repel one another and the walls of their container. Thus, the molecules of a gas are statically and uniformly distributed, trying to get as far apart as possible from one another and the vessel walls. This repulsion gives rise

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