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chemistry
physical chemistry

General Chemistry 9th edition Darrell Ebbing, Steven D. Gammon - Solutions

A given mass of gas occupies a volume of 435 mL at 25oC and 740 mmHg. What will be the new volume at STP?
A container is filled with 16.0 g of O2 and 14.0 g of N2. a. What is the volume of the container at STP? b. What is the partial pressure of the O2 gas? c. What are the mole fraction and the mole percent of the N2 in the mixture.
The ideal gas law relates four variables. An empirical gas law relates two variables, assuming the other two are constant. How many empirical gas laws can be obtained? Give statements of each.
Sulfur-containing compounds give skunks their potent smell. One of the principal smelly compounds in skunk spray is (E)-2-butene-1-thiol, C4H7S. a. What is the root-mean-square (rms) molecular speed of a gas molecule of this compound at 25oC? b. Using the value from part a, calculate how long it
Sulfur hexafluoride, SF6, is an extremely dense gas. How does its density compare with the density of air? Use a molar mass for air of 29.0 g/mol.
A rigid 1.0-L container at 75oC is fitted with a gas pressure gauge. A 1.0-mol sample of ideal gas is introduced into the container. a. What would the pressure gauge in the container be reading in mmHg? b. Describe the interactions in the container that are causing the pressure. c. Say the
The reaction 8H2(g) + S8(l) → 8H2S(g) is run at 125oC and a constant pressure of 12.0 atm. Assuming complete reaction, what mass of S8 would be required to produce 6.00 × 102 mL of H2S gas under these conditions?
Shown below are three containers of an ideal gas (A, B, and C), each equipped with a movable piston (assume that atmospheric pressure is 1.0 atm).a. How do the pressures in these containers compare?b. Are all the gases at the same temperature? If not, compare the temperatures.c. If you cooled each
A sample of natural gas is 85.2% methane, CH4, and 14.8% ethane, C2H6, by mass. What is density of this mixture at 18oC and 771 mmHg?
A sample of a breathing mixture for divers contained 34.3% helium, He; 51.7% nitrogen, N2; and 14.0% oxygen, O2 (by mass). What is the density of this mixture at 22oC and 755 mmHg?
A sample of sodium peroxide, Na2O2, was reacted with an excess of water. 2Na2O2(s) + 2H2O(l ) → 4NaOH(aq) + O2(g) All of the sodium peroxide reacted, and the oxygen was collected over water at 21oC. The barometric pressure was 771 mmHg. The apparatus was similar to that shown in Figure 5.20.
A sample of zinc metal was reacted with an excess of hydrochloric acid. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) All of the zinc reacted, and the hydrogen gas was collected over water at 17oC; the barometric pressure was 751 mmHg. The apparatus was similar to that shown in Figure 5.20, but the level
A mixture contained calcium carbonate, CaCO3, and magnesium carbonate, MgCO3. A sample of this mixture weighing 7.85 g was reacted with excess hydrochloric acid. The reactions are CaCO3(g) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g) MgCO3(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) + CO2(g) If the sample
Give the postulates of kinetic theory and state any evidence that supports them.
A mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are ZnS(s) + 2HCl(aq) → ZnCl2(aq) + H2S(g) PbS(s) + 2HCl(aq) → PbCl2(aq) + H2S(g) If the sample reacted completely and produced
A mixture of N2 and Ne contains equal moles of each gas and has a total mass of 10.0 g. What is the density of this gas mixture at 500 K and 15.00 atm? Assume ideal gas behavior.
A mixture of Ne and Ar gases at 350 K contains twice as many moles of Ne as of Ar and has a total mass of 50.0 g. If the density of the mixture is 4.00 g/L, what is the partial pressure of Ne?
An ideal gas with a density of 3.00 g/L has a pressure of 675 mmHg at 25oC. What is the root-mean-square speed of the molecules of this gas?
The root-mean-square speed of the molecules of an ideal gas at 25oC and a pressure of 2.50 atm is 5.00 × 102 m/s. What is the density of this gas?
Explain Boyle’s law in terms of the kinetic theory.
Explain why a gas appears to diffuse more slowly than average molecular speeds might suggest.
For what purpose is a manometer used? How does it work?
What is effusion? Why does a gas whose molecules have smaller mass effuse faster than one whose molecules have larger mass?
Shown below are two identical containers labeled A and B. Container A contains a molecule of an ideal gas, and container B contains two molecules of an ideal gas. Both containers are at the same temperature.a. How do the pressures in the two containers compare? Be sure to explain your answer.b.
Consider the box below that contains a single atom of an ideal gas.a. Assuming that this gas atom is moving, describe how it creates pressure inside the container.b. Now consider the two containers below, each at the same temperature. If we were to measure the gas pressure in each container, how
Using the concepts developed in this chapter, explain the following observations. a. Automobile tires are flatter on cold days. b. You are not supposed to dispose of aerosol cans in a fire. c. The lid of a water bottle pops off when the bottle sits in the sun. d. A balloon pops when you squeeze it.
What variables determine the height of the liquid in a manometer?
You have three identical flasks, each containing equal amounts of N2, O2, and He. The volume of the N2 flask is doubled, the O2 flask volume is halved, and the He flask volume is reduced to one-third of the original volume. Rank the flasks from highest to lowest pressure both before and after the
Consider the following gas container equipped with a movable piston.a. By what factor (increase by 1, decrease by 1.5, etc.) would you change the pressure if you wanted the volume to change from volume C to volume D?b. If the piston were moved from volume C to volume A, by what factor would the
A 3.00-L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0oC. a. How much (what fraction) of the total pressure in the flask is due to the N2? b. The flask is cooled and the pressure drops. What happens, if anything, to the mole fraction of the O2 at the lower
Consider the following setup, which shows identical containers connected by a tube with a valve that is presently closed. The container on the left has 1.0 mol of H2 gas; the container on the right has 1.0 mol of O2.Acceptable answers to some of these questions might be €œboth€
Two identical He-filled balloons, each with a volume of 20 L, are allowed to rise into the atmosphere. One rises to an altitude of 3000 m while the other rises to 6000 m. a. Assuming that the balloons are at the same temperature, which balloon has the greater volume? b. What information would you
You have a balloon that contains O2. What could you do to the balloon in order to double the volume? Be specific in your answers; for example, you could increase the number of moles of O2 by a factor of 2.
Three 25.0-L flasks are placed next to each other on a shelf in a chemistry stockroom. The first flask contains He at a pressure of 1.0 atm, the second contains Xe at 1.50 atm, and the third contains F2 and has a label that says 2.0 mol F2. Consider the following questions about these flasks. a.
A gas in a closed-tube manometer has a measured pressure of 0.047 atm. Calculate the pressure in mmHg.
The barometric pressure measured outside an airplane at 9 km (30,000 ft) was 259 mmHg. Calculate the pressure in kPa. Empirical Gas Laws
Suppose you had a 3.15-L sample of neon gas at 21oC and a pressure of 0.951 atm. What would be the volume of this gas if the pressure were increased to 1.292 atm while the temperature remained constant?
Starting with Boyle’s law (stated as an equation), obtain an equation for the final volume occupied by a gas from the initial volume when the pressure is changed at constant temperature.
You fill a balloon with helium gas to a volume of 2.68 L at 23oC and 789 mmHg. Now you release the balloon. What would be the volume of helium if its pressure changed to 632 mmHg but the temperature were unchanged?
You have a cylinder of argon gas at 19.8 atm pressure at 19oC. The volume of argon in the cylinder is 50.0 L. What would be the volume of this gas if you allowed it to expand to the pressure of the surrounding air (0.974 atm)? Assume the temperature remains constant.
A diving bell is a container open at the bottom. As the bell descends, the water level inside changes so that the pressure inside equals the pressure outside. Initially, the volume of air is 8.58 m3 at 1.020 atm and 20oC. What is the volume at 1.212 atm and 20oC?
A McLeod gauge measures low gas pressures by compressing a known volume of the gas at constant temperature. If 315 cm3 of gas is compressed to a volume of 0.0457 cm3 under a pressure of 2.51 kPa, what was the original gas pressure?
If 456 dm3 of krypton at 101 kPa and 21oC is compressed into a 27.0-dm3 tank at the same temperature, what is the pressure of krypton in the tank?
A sample of nitrogen gas at 18oC and 760 mmHg has a volume of 3.92 mL. What is the volume at 0oC and 1 atm of pressure?
A mole of gas at 0oC and 760 mmHg occupies 22.41 L. What is the volume at 20oC and 760 mmHg?
Helium gas, He, at 22oC and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?
An experiment called for 4.83 L of sulfur dioxide, SO2, at 0oC and 1.00 atm. What would be the volume of this gas at 25oC and 1.00 atm?
A vessel containing 39.5 cm3 of helium gas at 25oC and 106 kPa was inverted and placed in cold ethanol. As the gas contracted, ethanol was forced into the vessel to maintain the same pressure of helium. If this required 7.7 cm3 of ethanol, what was the final temperature of the helium?
The volume occupied by a gas depends linearly on degrees Celsius at constant pressure, but it is not directly proportional to degrees Celsius. However, it is directly proportional to kelvins. What is the difference between a linear relationship and a direct proportion?
A sample of 62.3 cm3 of argon gas at 18oC was contained at a pressure of 155 kPa in a J shaped tube with mercury. Later the temperature changed. When the mercury level was adjusted to give the same pressure of argon, the gas volume changed to 61.2 cm3. What was the final temperature of the argon?
A bacterial culture isolated from sewage produced 35.5 mL of methane, CH4, at 31oC and 753 mmHg. What is the volume of this methane at standard temperature and pressure (0oC, 760 mmHg)?
Pantothenic acid is a B vitamin. Using the Dumas method, you find that a sample weighing 71.6 mg gives 3.84 mL of nitrogen gas at 23oC and 785 mmHg. What is the volume of nitrogen at STP?
In the presence of a platinum catalyst, ammonia, NH3, burns in oxygen, O2, to give nitric oxide, NO, and water vapor. How many volumes of nitric oxide are obtained from one volume of ammonia, assuming each gas is at the same temperature and pressure?
Methanol, CH3OH, can be produced in industrial plants by reacting carbon dioxide with hydrogen in the presence of a catalyst. Water is the other product. How many volumes of hydrogen are required for each volume of carbon dioxide when each gas is at the same temperature and pressure?
Starting from the ideal gas law, prove that the volume of a mole of gas is inversely proportional to the pressure at constant temperature (Boyle’s law).
Starting from the ideal gas law, prove that the volume of a mole of gas is directly proportional to the absolute temperature at constant pressure (Charles’s law).
A cylinder of oxygen gas contains 91.3 g O2. If the volume of the cylinder is 8.58 L, what is the pressure of the O2 if the gas temperature is 21oC?
In an experiment, you fill a heavy-walled 5.00-L flask with methane gas, CH4. If the flask contains 7.13 g of methane at 19oC, what is the gas pressure?
An experiment calls for 3.50 mol of chlorine, Cl2. What volume will this be if the gas volume is measured at 34oC and 4.00 atm?
Explain how you would set up an absolute temperature scale based on the Fahrenheit scale, knowing that absolute zero is 273.15oC.
According to your calculations, a reaction should yield 5.67 g of oxygen, O2. What do you expect the volume to be at 23oC and 0.985 atm?
The maximum safe pressure that a certain 4.00-L vessel can hold is 3.50 atm. If the vessel contains 0.410 mol of gas, what is the maximum temperature (in degrees Celsius) to which this vessel can be subjected?
A 2.50-L flask was used to collect a 5.65-g sample of propane gas, C3H8. After the sample was collected, the gas pressure was found to be 741 mmHg. What was the temperature of the propane in the flask?
What is the density of ammonia gas, NH3, at 31oC and 751 mmHg? Obtain the density in grams per liter.
Calculate the density of hydrogen sulfide gas, H2S, at 56oC and 967 mmHg. Obtain the density in grams per liter.
Butane, C4H10, is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.897 atm and 24oC. Give the answer in grams per liter.
Chloroform, CHCl3, is a volatile (easily vaporized) liquid solvent. Calculate the density of chloroform vapor at 98oC and 797 mmHg. Give the answer in grams per liter.
A chemist vaporized a liquid compound and determined its density. If the density of the vapor at 90oC and 753 mmHg is 1.585 g/L, what is the molecular mass of the compound?
You vaporize a liquid substance at 100oC and 755 mmHg. The volume of 0.548 g of vapor is 237 mL. What is the molecular mass of the substance?
A 2.56-g sample of a colorless liquid was vaporized in a 250-mL flask at 121oC and 786 mmHg. What is the molecular mass of this substance?
Starting with Charles’s law (stated as an equation), obtain an equation for the final volume of a gas from its initial volume when the temperature is changed at constant pressure.
A 2.30-g sample of white solid was vaporized in a 345- mL vessel. If the vapor has a pressure of 985 mmHg at 148oC, what is the molecular mass of the solid?
Ammonium chloride, NH4Cl, is a white solid. When heated to 325C, it gives a vapor that is a mixture of ammonia and hydrogen chloride. NH4Cl(s) → NH3(g) + HCl(g) Suppose someone contends that the vapor consists of NH4Cl molecules rather than a mixture of NH3 and HCl. Could you decide between
Phosphorus pentachloride, PCl5, is a white solid that sublimes (vaporizes without melting) at about 100oC. At higher temperatures, the PCl5 vapor decomposes to give phosphorus trichloride, PCl3, and chlorine, Cl2. PCl5(g) → PCl3(g) + Cl2(g) How could gas-density measurements help to establish
Calcium carbide reacts with water to produce acetylene gas, C2H2. CaC2(s) + 2H2O(l) → Ca(OH)2(aq) + C2H2(g) Calculate the volume (in liters) of acetylene produced at 26oC and 684 mmHg from 0.050 mol CaC2 and excess H2O.
Magnesium metal reacts with hydrochloric acid to produce hydrogen gas, H2. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) Calculate the volume (in liters) of hydrogen produced at 33oC and 665 mmHg from 0.0840 mol Mg and excess HCl.
Lithium hydroxide, LiOH, is used in spacecraft to recondition the air by absorbing the carbon dioxide exhaled by astronauts. The reaction is 2LiOH(s) + CO2(g) → Li2CO3(s) + H2O(l ) What volume of carbon dioxide gas at 218C and 781 mmHg could be absorbed by 327 g of lithium hydroxide?
Magnesium burns in air to produce magnesium oxide, MgO, and magnesium nitride, Mg3N2. Magnesium nitride reacts with water to give ammonia. Mg3N2(s) + 6H2O(l ) → 3Mg(OH)2(s) + 2NH3(g) What volume of ammonia gas at 24oC and 753 mmHg will be produced from 4.56 g of magnesium nitride?
Urea, NH2CONH2, is a nitrogen fertilizer that is manufactured from ammonia and carbon dioxide. 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l ) What volume of ammonia at 25oC and 3.00 atm is needed to produce 908 g (2 lb) of urea?
Nitric acid is produced from nitric oxide, NO, which in turn is prepared from ammonia by the Ostwald process: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) What volume of oxygen at 35oC and 2.15 atm is needed to produce 50.0 g of nitric oxide?
Ammonium sulfate is used as a nitrogen and sulfur fertilizer. It is produced by reacting ammonia with sulfuric acid. Write the balanced equation for the reaction of gaseous ammonia with sulfuric acid solution. What volume (in liters) of ammonia at 15oC and 1.15 atm is required to produce 150.0 g of
State Avogadro’s law in words. How does this law explain the law of combining volumes? Use the gas reaction N2 + 3H2 → 2NH3 as an example in your explanation.
Sodium hydrogen carbonate is also known as baking soda. When this compound is heated, it decomposes to sodium carbonate, carbon dioxide, and water vapor. Write the balanced equation for this reaction. What volume (in liters) of carbon dioxide gas at 77oC and 756 mmHg will be produced from 26.8 g of
Calculate the total pressure (in atm) of a mixture of 0.0200 mol of helium, He, and 0.0100 mol of hydrogen, H2, in a 2.50-L flask at 10oC. Assume ideal gas behavior.
Calculate the total pressure (in atm) of a mixture of 0.0300 mol of helium, He, and 0.0200 mol of oxygen, O2, in a 4.00-L flask at 20C. Assume ideal gas behavior.
A 200.0-mL flask contains 1.03 mg O2 and 0.56 mg He at 15oC. Calculate the partial pressures of oxygen and of helium in the flask. What is the total pressure?
The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.200 atm of oxygen and a total pressure of 3.00 atm, calculate the mass of helium in 10.0 L of the gas mixture at 20oC.
The gas from a certain volcano had the following composition in mole percent (that is, mole fraction × 100): 65.0% CO2, 25.0% H2, 5.4% HCl, 2.8% HF, 1.7% SO2, and 0.1% H2S. What would be the partial pressure of each of these gases if the total pressure of volcanic gas were 760 mmHg?
In a series of experiments, the U.S. Navy developed an undersea habitat. In one experiment, the mole percent composition of the atmosphere in the undersea habitat was 79.0% He, 17.0% N2, and 4.0% O2. What will the partial pressure of each gas be when the habitat is 58.8 m below sea level, where the
Formic acid, HCHO2, is a convenient source of small quantities of carbon monoxide. When warmed with sulfuric acid, formic acid decomposes to give CO gas. HCHO2(l ) → H2O(l ) + CO(g) If 3.85 L of carbon monoxide was collected over water at 25oC and 689 mmHg, how many grams of formic acid were
An aqueous solution of ammonium nitrite, NH4NO2, decomposes when heated to give off nitrogen, N2. NH4NO2(s) → 2H2O(g) + N2(g) This reaction may be used to prepare pure nitrogen. How many grams of ammonium nitrite must have reacted if 3.75 dm3 of nitrogen gas was collected over water at 26C and
Calculate the rms speeds of N2 molecules at 25oC and at 125oC. Sketch approximate curves of the molecular speed distributions of N2 at 25oC and at 125oC.
Calculate the rms speed of Br2 molecules at 23oC and 1.00 atm. What is the rms speed of Br2 at 23oC and 1.50 atm?
Uranium hexafluoride, UF6, is a white solid that sublimes (vaporizes without melting) at 57oC under normal atmospheric pressure. The compound is used to separate uranium isotopes by effusion. What is the rms speed (in m/s) of a uranium hexafluoride molecule at 57oC?
For a spacecraft or a molecule to leave the moon, it must reach the escape velocity (speed) of the moon, which is 2.37 km/s. The average daytime temperature of the moon’s surface is 365 K. What is the rms speed (in m/s) of a hydrogen molecule at this temperature? How does this compare with the
At what temperature would CO2 molecules have an rms speed equal to that of H2 molecules at 25oC?
At what temperature does the rms speed of O2 molecules equal 400. m/s?
What is the ratio of rates of effusion of N2 and O2 under the same conditions?
Obtain the ratio of rates of effusion of H2 and H2Se under the same conditions.
If 0.10 mol of i2 vapor can effuse from an opening in a heated vessel in 39 s, how long will it take 0.10 mol H2 to effuse under the same conditions?

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