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chemistry for engineering students

Chemistry For Engineering Students 4th Edition Lawrence S. Brown, Tom Holme - Solutions

Shrimp are usually labeled with a “count” that indicates the average number of shrimp per pound. The bigger the shrimp, the smaller the count. Suppose that your supermarket is offering 20-count shrimp for $5.99 per pound. How much should you expect to pay for one dozen shrimp?Strategy We can
How many significant figures are there in each of the following? (a) 0.136 m,(b) 0.0001050 g,(c) 2.700 × 10–3 nm,(d) 6 × 10–4 L, (e) 56003 cm3
How many significant figures are present in these measured quantities? (a) 1374 kg, (b) 0.00348 s, (c) 5.619 mm, (d) 2.475 × 10–3 cm, (e) 33.1 mL
The chlorine present in PVC has two stable isotopes. 35Cl with a mass of 34.97 amu makes up 75.77% of the natural chlorine found. The other isotope is 37Cl, whose mass is 36.95 amu. What is the atomic weight of chlorine?Strategy To determine the atomic weight, we must calculate the average mass
We cannot generally produce a polymer by simply mixing a large sample of the desired monomers. Instead, additional compounds called initiators or catalysts are almost always needed to start a polymerization. One polymerization catalyst is diethylaluminum chloride, Al(C2H5)2Cl. How many of each type
A 245.3-g sample of glutamic acid, C5H9NO4, is recovered from an experiment using fermentation to convert biomass. How many moles of C5H9NO4 are in this sample? How many molecules is this?Strategy We are asked to convert from mass to moles. So we must determine the molar mass of the substance and
One goal of biomass conversion is the development of feedstocks, chemicals that can be easily converted to raw materials for chemical processes like the synthesis of polymers. One important feedstock molecule that can be derived from biomass is 2-propanol, C3H7OH. If 423 moles of the compound are
In Section 3.2, we considered the reaction between hydrogen and oxygen to form water. How many grams of water can be produced if sufficient hydrogen reacts with 26.0 g of oxygen?Strategy First, it will help if we recognize that this is a reaction stoichiometry problem. Two signs of this are that it
A solution of hydrochloric acid contains 5.22 g of HCl. When it is allowed to react with 3.25 g of solid K2CO3, the products are KCl, CO2, and H2O. Which reactant is in excess?Strategy As for any reaction stoichiometry problem, we should start with a balanced equation. One way to proceed from there
In Example Problem 4.3, we used the reaction that produces P4S3, one of the reactants in the combustion of a match:If 28.2 g of P4 is allowed to react with 18.3 g of S8, which is the limiting reactant?Strategy We can choose either reactant and determine how much of the other reactant is required to
MTBE (methyl tert-butyl ether) has been used as an additive in gasoline. The compound is produced by reacting methanol and isobutene, according to the following equation:If 45.0 kg of methanol is allowed to react with 70.0 kg of isobutene, what is the maximum mass of MTBE that can be
The Draco thrusters on SpaceX’s Dragon spacecraft are based on the following reaction between monomethylhydrazine (CH6N2) and dinitrogen tetroxide (N2O4):If either reactant is in excess, unnecessary mass will be added to the craft, so a stoichiometric mixture is desired. What mass of each
The Solvay process is important in the commercial production of sodium carbonate (Na2CO3), which is used in the manufacture of most glass. The last step in the Solvay process is the conversion of NaHCO3 (sodium bicarbonate, or baking soda) to Na2CO3 by heating:In a laboratory experiment, a student
The fuel hydrazine, N2H4, can be produced by the reaction of solutions of sodium hypochlorite and ammonia. The relevant chemical equation isIf 750.0 mL of 0.806 M NaClO is mixed with excess ammonia, how many moles of hydrazine can be formed? If the final volume of the resulting solution is 1.25 L,
MTBE, C5H12O, is one of the additives that replaced tetraethyl-lead in gasoline. (See Example Problem 4.6 and Section 4.6.) How many moles of O2 are needed for the complete combustion of 1.50 mol of MTBE?Example Problem 4.6MTBE (methyl tert-butyl ether) has been used as an additive in gasoline. The
Many common titrations involve the reaction of an acid with a base. If 24.75 mL of 0.503 M NaOH solution is used to titrate a 15.00-mL sample of sulfuric acid, H2SO4, what is the concentration of the acid?Strategy A titration problem is an applied stoichiometry problem, so we will need a balanced
Blood alcohol levels are usually reported in mass percentages: A level of 0.10 means that 0.10 g of alcohol (C2H5OH) was present in 100 g of blood. This is just one way of expressing the concentration of alcohol dissolved in the blood. Other concentration units could be used. Find the molarity of
One way of determining blood alcohol levels is by performing a titration on a sample of blood. In this process, the alcohol from the blood is oxidized by dichromate ions (Cr2O7 2-) according to the following net ionic equation:A 10.00-g sample of blood was drawn from a patient, and 13.77 mL of
Ammonium sulfate ((NH4)2SO4) is a common fertilizer that can be produced by the reaction of ammonia (NH3) with sulfuric acid (H2SO4). Each year about 1 × 1010 kg of ammonium sulfate is produced worldwide. How many kilograms of ammonia would be needed to generate this quantity of (NH4)2SO4? (Assume
Aluminum chloride (AlCl3) is used as a catalyst in the production of polyisobutylene, which is used in automobile tires. Scrap aluminum metal reacts with chlorine gas (Cl2) to produce AlCl3. Suppose that 2.70 g of Al and 7.10 g of Cl2 are mixed. What is the maximum mass of AlCl3 that could be
In the cold vulcanization of rubber, disulfur dichloride (S2Cl2) is used as a source of sulfur atoms, and those sulfur atoms form “bridges,” or cross-links, between polymer chains. S2Cl2 can be produced by reacting molten sulfur (S8(ℓ)) with chlorine (Cl2(g)). What is the maximum mass of
A quality control technician needs to determine the percentage of arsenic (As) in a particular pesticide. The pesticide is dissolved, and all of the arsenic present is converted to arsenate ions (AsO4 3-). Then the amount of AsO4 3- is determined by titrating with a solution containing silver
Calcium carbonate (limestone, CaCO3) dissolves in hydrochloric acid, producing water and carbon dioxide as shown in the following unbalanced net ionic equation:Suppose 5.0 g of CaCO3 is added to 700. mL of 0.10 M HCl. What is the maximum mass of CO2 that could be formed? What would the final
Iron metal can be refined from the mineral hematite (Fe2O3). One way of converting the mineral to iron is to react it with carbon monoxide, as shown below:Because the hematite is obtained from various ores, it is usually not in a pure form. Suppose an iron manufacturer has 2.00 × 105 kg of ore
Calcium sulfate is the essential component of plaster and sheet rock. Waste calcium sulfate can be converted into quicklime, CaO, by reaction with carbon at high temperatures. The following two equations represent a sequence of reactions that might take place:What mass of sulfur dioxide could be
Iron–aluminum alloys are useful in some applications because they become magnetized in a magnetic field but are easily demagnetized when the field is removed. The composition of an iron–aluminum alloy can be determined chemically by reacting it with hydrochloric acid:When a 7.264-g sample of a
A mixture of methane (CH4) and propane (C3H8) has a total mass of 29.84g. When the mixture is burned completely in excess oxygen, the CO2 and H2O products have a combined mass of 142.97g. Calculate the mass of methane in the original mixture.
A mixture of hydrochloric and sulfuric acids is prepared so that it contains 0.100 M HCl and 0.200 M H2SO4. What volume of 0.250 M NaOH would be required to completely neutralize all of the acid in 425 mL of this solution?
A solution contains both Ca2+ and Pb2+ ions. A 50.0-mL sample of this solution was treated with 0.528 M NaF, and 53.8 mL of the NaF solution was needed to precipitate all of the Ca2+ and Pb2+ as CaF2(s) and PbF2(s). The precipitate was dried and weighed and had a total mass of 3.141g. What was the
The carbon dioxide exhaled by astronauts must be removed from the air. One way to do this is through the use of CO2 “scrubbers” based on metal hydroxides. CO2 reacts with the hydroxide to form the corresponding metal carbonate and water. Because these scrubbers need to be sent into space,
You are designing a process for a wastewater treatment facility intended to remove aqueous HCl from the input water. Several bases are being considered for use, and their costs are listed in the table below. If cost is the primary concern, which base would you recommend using? Use stoichiometric
Iron(II) ions react with phenanthroline (C12H8N2) to form a complex ion with the general formula Fex(C12H8N2)y 2x+. A student uses the method of continuous variation to determine the number of phenanthroline molecules bound to each iron ion (i.e., the values of x and y in the formula). The complex
Chromium metal is found in ores as an oxide, Cr2O3. This ore can be converted to metallic Cr by the Goldschmidt process, Cr2O3(s) + 2 Al(s) → 2 Cr (ℓ) + Al2O3(s). Suppose that you have 4.5 tons of chromium (III) oxide. Describe how you would determine how much aluminum metal you would need to
Hydrochloric acid reacts with many metals to form hydrogen gas, H2. If you needed to produce hydrogen as a source of fuel in some design, how would you determine which metal—Mg, Al, or Zn—would produce the greatest amount of hydrogen per gram of metal? Describe the steps you would need to take
Benzopyrene is a hydrocarbon that is known to cause cancer. Combustion analysis (see Problem 4.108) of a 2.44-g sample of this compound shows that combustion produces 8.54 g of CO2 and 1.045 g of H2O. What is the empirical formula of benzopyrene?Data from problem 4.108Elemental analysis is
People sometimes use the terms natural gas and methane interchangeably. Explain why this is not completely correct.
For homes or businesses in some rural areas, natural gas pipelines may not be available. In such cases, methane might be obtained in a compressed gas cylinder. A common laboratory cylinder of methane has a volume of 49.0 L and is filled to a pressure of 154 atm. Suppose that all of the CH4 from
What gases, other than methane, are most likely to be found in natural gas when it is first recovered in mining operations?
What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?
About 60% of annual U.S. ethane production is recovered during the processing of natural gas. A sample of ethane (C2H6) gas has a volume of 575 cm3 at 752 torr and 72°F. What is the mass of ethane in this sample?Strategy We are trying to find the mass of a sample of gas. If we knew how many moles
How does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?
Natural gas wells are not the only source of gases emerging from the earth. Volcanoes, for example, are a naturally occurring source of various gases. A scientist tries to generate a mixture of gases similar to those found in a volcano by introducing 15.0 g of water vapor, 3.5 g of SO2, and 1.0 g
An experiment is designed to test a component in a natural gas processing plant. To mimic the raw natural gas, a mixture is prepared with the mole fractions given in the following table.If the desired total pressure is 750 torr, what should the partial pressures be? If the gas is to be in a 15.0-L $Gas Mole fraction CH4 0.865 CO 0.029 CH6 0.072 C3H8 0.034$
What is meant by horizontal drilling, and how does it differ from traditional drilling methods for natural gas and oil recovery?
Hydrogen sulfide, H2S, is present in many oil products, including natural gas from many sources. The removal of this sulfur-containing molecule involves several steps, including the following reaction:Studying this reaction in the laboratory requires extra safety precautions because of the toxicity
Use the Internet to determine what areas of the United States have made the widest use of hydraulic fracturing. Is the current production of natural gas from these areas smaller, greater, or about the same as it was 5 years ago?
One observable property of gases is the variability of density based on conditions. Use this observation to explain why hot air balloons rise.
If you are pounding a nail and miss it, the hammer may dent the wood, but it does not penetrate it. Use the concept of pressure to explain this observation.
How do gases exert atmospheric pressure?
Why do mountain climbers need to wear breathing apparatuses at the tops of high mountains such as Denali in Alaska?
If you had a liquid whose density was half that of mercury, how tall would you need to build a barometer to measure atmospheric pressure in a location where the record pressure recorded was 750 mm Hg?
Water has a density that is 13.6 times less than that of mercury. If an undersea vessel descends to 1.5 km, how much pressure does the water exert in atm?
Does the vacuum above the mercury in the column of a barometer affects the reading it gives? Why or why not?
Gas pressures can be expressed in units of mm Hg, atm, torr, and kPa. Convert these pressure values.(a) 722 mm Hg to atm, (b) 1.25 atm to mm Hg, (c) 542 mm Hg to torr, (d) 745 mm Hg to kPa, (e) 708 kPa to atm
If the atmospheric pressure is 97.4 kPa, how much is it in mm Hg? In atm?
Why do your ears “pop” on occasion when you swim deep underwater?
When helium escapes from a balloon, the balloon’s volume decreases. Based on your intuition about stretching rubber, explain how this observation is consistent with the gas law.
A gas has an initial volume of 39 mL at an unknown pressure. If the same sample occupies 514 mL at 720 torr, what was the initial pressure?
When you buy a Mylar® balloon in the winter months in colder places, the shopkeeper will often tell you not to worry about it losing its shape when you take it home (outside) because it will return to shape once inside. What behavior of gases is responsible for this advice?
Calculate the missing variable in each of these sets:V1 = 2.0 L, T1 = 15°C, V2 =? T2 = 34°CV1 =? T1 = 149°C, V2 = 310 mL, T2 = 54°CV1 = 150 L, T1 = 180 K, V2 = 57 L, T2 =?
A gas bubble forms inside a vat containing a hot liquid. If the bubble is originally at 68°C and a pressure of 1.6 atm with a volume of 5.8 mL, what will its volume be if the pressure drops to 1.2 atm and the temperature drops to 31°C?
A bicycle tire is inflated to a pressure of 3.74 atm at 15°C. If the tire is heated to 35°C, what is the pressure in the tire? Assume the tire volume doesn’t change.
A balloon filled with helium has a volume of 1.28 × 103 L at sea level where the pressure is 0.998 atm and the temperature is 31°C. The balloon is taken to the top of a mountain where the pressure is 0.753 atm and the temperature is -25°C. What is the volume of the balloon at the top of the
How many moles of an ideal gas are there if the volume of the gas is 158 L at 14°C and a pressure of 89 kPa?
A newly discovered gas has a density of 2.39 g/L at 23.0°C and 715 mm Hg. What is the molar mass of the gas?
Calculate the mass of each of the following gases at STP:(a) 1.4 L of SO2, (b) 3.5 × 105 L of CO2
What are the densities of the following gases at STP?(a) CF2Cl2,(b) CO2, (c) HCl
Cylinders of compressed gases are often labeled to show how many “SCF” or “standard cubic feet” of gas they contain. 1 SCF of gas occupies a volume of 1 ft3 at a standard temperature and pressure of 0°C and 1 atm. A particular cylinder weighs 122 lb. when empty and 155 lb. when filled with
Define the term partial pressure.
Define the term mole fraction.
How does the mole fraction relate to the partial pressure?
What is the total pressure exerted by a mixture of 1.50 g of H2 and 5.00 g of N2 in a 5.00-L vessel at 25°C?
What is the total pressure (in atm) of a 15.0-L container at 28.0°C that contains 3.5 g of N2, 4.5 g of O2, and 13.0 g of Cl2?
For a gas sample whose total pressure is 740 torr, what are the partial pressures if the gas present consists of 1.3 mol of N2, 0.33 mol of O2, and 0.061 mol of Ar?
A sample containing only NO2 and SO2 has a total pressure of 120. torr. Measurements show that the partial pressure of NO2 is 43 torr. If the vessel has a volume of 800.0 mL and the temperature is 22.0°C, how many moles of each gas are present?
A sample of gas is made up entirely of carbon dioxide and water, and there are 259 moles of CO2 and 513 moles of water. If the total pressure of the sample is 21 atm, what is the partial pressure of each gas?
A sample of a smokestack emission was collected into a 1.25-L tank at 752 mm Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by each gas?
Air is often modeled as dry air, ignoring the water present. The mole fractions of nitrogen and oxygen in dry air are 0.7808 and 0.2095, respectively. If the atmospheric pressure outside is 0.944 atm and the pressure associated with water is 0.039 atm, what are the partial pressures of nitrogen and
In an experiment, a mixture of gases occupies a volume of 30.00 L at a temperature of 122.5°C. The mixture contains 14.0 g of water, 11.5 g of oxygen, and 37.3 g of nitrogen. Calculate the total pressure and the partial pressure of each gas.
An experiment is being carried out to test the removal of sulfur dioxide from gases being released by a power plant. The initial sample, which contains only carbon dioxide and sulfur dioxide, occupies a volume of 35 L at a temperature of 41°C and a pressure of 715 torr. After all of the SO2 has
Use the web to determine the range of partial pressures that oxygen sensors must measure in the exhaust manifold of automobile engines. Why is it important for an engineer to know the amount of oxygen in an exhaust stream?
Use the web to research the types of fuel-to-air mixtures present in regular consumer driven automobiles. Calculate the partial pressures of the gases present based on the information you find.
HCl(g) reacts with ammonia gas, NH3(g), to form solid ammonium chloride. If a sample of ammonia occupying 250 mL at 21°C and a pressure of 140 torr is allowed to react with excess HCl, what mass of NH4Cl will form?
Hydrogen gas is generated when acids come into contact with certain metals. When excess hydrochloric acid reacts with 2.5 g of Zn (the metal product is Zn2+), what volume of hydrogen gas is collected at a pressure of 0.93 atm and a temperature of 22°C?
The first step in processing zinc metal from its ore, ZnS, is to react it with O2 according to the reactionIf 620 kg of ZnS is to be reacted, what volume of oxygen at 0.977 atm and 34.0°C is needed (at a minimum) to carry out this reaction? 2 ZnS(s) + 3 O₂(g) →2 ZnO(s) + 2 SO₂(g)
If you need 400.0 mL of hydrogen gas to conduct an experiment at 20.5°C and 748 torr, how many grams of Zn should be reacted with excess HCl to obtain this much gas?
What volume of oxygen at 24°C and 0.88 atm is needed to completely react via combustion with 45 g of methane gas?
If tetraborane, B4H10, is treated with pure oxygen, it burns to give B2O3 and H2O:If a 0.050-g sample of tetraborane burns completely in O2, what will be the pressure of the gaseous water in a 4.25-L flask at 30.0°C? 2 B4H10(s) + 11 O₂(g) →4 B₂O3(s) + 10 H₂O(g)
In Example Problem 5.1, we considered a CH4 storage tank with a volume of 49.0l. When empty, the tank has a mass of 55.85 kg, and when filled, its mass is 62.07 kg.Calculate the pressure of CH4 in the tank at an ambient temperature of 21°C using both the ideal gas equation and the van der Waals
N2O5 is an unstable gas that decomposes according to the following reaction:What would be the total pressure of gases present if a 10.0-L container at 22.0°C begins with 0.400 atm of N2O5 and the gas completely decomposes? 2 N₂O,(g) →4 NO₂(g) + O₂(g)
One way to generate oxygen is to heat potassium chlorate, KClO3. (The other product is potassium chloride.) If 386 mL of oxygen at 41°C and 97.8 kPa is generated by this reaction, what is the minimum mass of KClO3 used?
What volume of hydrogen gas, in liters, is produced by the reaction of 3.43 g of iron metal with 40.0 mL of 2.43 M HCl? The gas is collected at 2.25 atm of pressure and 23°C. The other product is FeCl2.
Magnesium will burn in air to form both Mg3N2 and MgO. What mass of each product would be found if burning a 3.11-g sample of magnesium to completion produces a combined total of 5.09 g of the two products?
During a collision, automobile air bags are inflated by the N2 gas formed by the explosive decomposition of sodium azide, NaN3:What mass of sodium azide would be needed to inflate a 30.0-L bag to a pressure of 1.40 atm at 25°C? 2 NaN3 → 2 Na + 3 N₂
Automakers are always investigating alternative reactions for the generation of gas to inflate air bags, in part because the sodium produced in the decomposition of NaN3 (see Problem 5.59) presents safety concerns. One system that has been considered is the oxidation of graphite by strontium
As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni (CO)4, which is a gas at temperatures above about 316 k.A 2.00-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the
Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminum chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, ADN rapidly decomposes to produce a gaseous mixture of N2, O2, and H2O. (This is not
Clouds of hydrogen molecules have been detected deep in interstellar space. It is estimated that these clouds contain about 1 × 1010 hydrogen molecules per m3 and have a temperature of just 25k. Using these data, find the approximate pressure in such a cloud. NASA
State the postulates of the kinetic theory of gases.
Place these gases in order of increasing average molecular speed at 25°C: Kr, CH4, N2, CH2Cl2.

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