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chemistry for engineering students

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

How many O atoms are present in 214 g of mannose (C6H12O6)?
A sample of H2C2O4 · 2H2O of mass 3.35 g is heated to drive off the waters of hydration (designated separately in the chemical formula). What mass of H2C2O4 remains once the water has been removed by heating?
An average person inhales roughly 2.5 g of O2 in a minute. How many molecules of oxygen are inhaled in(a) 1 minute, (b) 1 hour,(c) 1 day by an average person?
Determine the simplest formulas of the following compounds.(a) The food enhancer monosodium glutamate (MSG), which has the composition 35.51% C, 4.77% H, 37.85% O, 8.29% N, and 13.60% Na; (b) Zircon, a diamond-like mineral, which has the composition 34.91% O, 15.32% Si, and 49.76% Zr; (c)
The composition of materials such as alloys can be described in terms of mole percentage (mol%), atom percentage (at%), or weight percentage (wt%). Carry out the following conversions among these units.(a) 60 wt% Cu and 40 wt% Al to at%,(b) 25 mol% NiO and 75 mol% MgO to wt%,(c) 40 wt% MgO and 60
Copper can have improved wear resistance if alloyed with ceramic alumina, Al2O3. If a copper alloy has 8.5 wt% Al2O3, what is its composition in mol%?
Calculate the molarity of each of the following solutions.(a) 1.45 mol HCl in 250. mL of solution (b) 14.3 mol NaOH in 3.4 L of solution(c) 0.341 mol KCl in 100.0 mL of solution (d) 250 mol NaNO3 in 350 L of solution
What is the molarity of each ion present in aqueous solutions prepared by dissolving 20.00 g of the following compounds in water to make 4.50 L of solution?(a) Cobalt (III) chloride, (b) Nickel (III) sulfate,(c) Sodium permanganate, (d) Iron (II) bromide
How many moles of solute are present in each of these solutions?(a) 48.0 mL of 3.4 M H2SO4(b) 1.43 mL of 5.8 M KNO3(c) 3.21 L of 0.034 M NH3(d) 1.9 × 103 L of 1.4 × 10–5 M NaF
How many grams of solute are present in each of these solutions?(a) 37.2 mL of 0.471 M HBr (b) 113.0 L of 1.43 M Na2CO3(c) 21.2 mL of 6.8 M CH3COOH (d) 1.3 × 10–4 L of 1.03 M H2SO3
Determine the final molarity for the following dilutions.(a) 24.5 mL of 3.0 M solution diluted to 100.0 mL(b) 15.3 mL of 4.22 M solution diluted to 1.00 L(c) 1.45 mL of 0.034 M solution diluted to 10.0 mL(d) 2.35 L of 12.5 M solution diluted to 100.0 L
Determine the initial volume (in mL) needed to generate each of the following desired solutions by dilution.(a) 10.0 L of 0.45 M solution from 3.0 M solution(b) 1.50 L of 1.00 M solution from 11.7 M solution(c) 100.0 mL of 0.025 M solution from 1.15 M solution(d) 50.0 mL of 3.3 × 10–4 M solution
Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume of concentrated sulfuric acid required to prepare 2.50 L of 1.50 M H2SO4 solution.
Magnesium is lighter than other structural metals, so it is increasingly important in the design of more efficient vehicles. Mg2+ ions are present in seawater, and the metal is often prepared by “harvesting” these ions and converting them to Mg metal. The average magnesium content of the oceans
Carbon dioxide is just one of many greenhouse gases in the atmosphere. What property makes a gas a greenhouse gas?
For the reaction of nitrogen, N2, and hydrogen, H2, to form ammonia, NH3, a student is attempting to draw a particulate diagram, as shown below. Did the student draw a correct representation of the reaction? If not, what was the error the student made? = N c = H
The picture shown depicts the species present at the start of a combustion reaction between methane, CH4, and oxygen, O2.(a) Draw the resulting state after this set of reactants has reacted as far as possible. (b) Use the drawings to explain the stoichiometry represented in the balanced chemical
The particulate drawing shown represents an aqueous solution of an acid HA, where A might represent an atom or group of atoms. Is HA a strong acid or a weak acid?Explain how you can tell from the picture. = 0 = A = H
Nitric acid (HNO3) can be produced by the reaction of nitrogen dioxide (NO2) and water. Nitric oxide (NO) is also formed as a product. Write a balanced chemical equation for this reaction. Nitric acid, HNO3
When a solution is diluted, solvent is added but solute is not. Explain how this idea leads to the equation frequently used in dilution calculations, M1V1 = M2V2.
One step in the enrichment of uranium for use in nuclear power plants involves the reaction of UO2 with hydrofluoric acid (HF) solution. The products are solid UF4 and water. Write a balanced chemical equation for this reaction.
Pyridine has the molecular formula C5H5N. When pyridine reacts with O2, the products are CO2, H2O, and N2. Write a balanced equation for this reaction.
Hydrogen cyanide (HCN) is extremely toxic, but it is used in the production of several important plastics. In the most common method for producing HCN, ammonia (NH3) and methane (CH4) react with oxygen (O2) to give HCN and water. Write a balanced chemical equation for this reaction. Hydrogen
Pyrrole has the molecular formula C4H5N. When pyrrole reacts with O2, the products are CO2, H2O, and N2. Write a balanced equation for this reaction.
Adipic acid is used in the production of nylon, so it is manufactured in large quantities. The most common method for the preparation of adipic acid is the reaction of cyclohexane with oxygen. Balance the skeleton equation shown below. + O₂ cyclohexane HO adipic acid OH + H₂O
Many chemical reactions take place in the catalytic converter of a car. In one of these reactions, nitric oxide (NO) reacts with ammonia (NH3) to give nitrogen (N2) and water. Write a balanced equation for this reaction.
Calcium carbonate (limestone, CaCO3) dissolves in hydrochloric acid, producing water and carbon dioxide. An unbalanced net ionic equation for this reaction is given below. Balance it. CaCO3(s) + H3O+ (aq) → H,O() + CO,(g)+Ca+(aq)
Methyl cyanoacrylate is the chemical name for the substance sold as Super Glue, and it has the chemical formula C5H5NO2. Calculate the number of molecules of this substance in a 1.0-ounce tube of Super Glue, assuming that the glue is 80% methyl cyanoacrylate by mass.
A low-grade form of iron ore is called taconite, and the iron in the ore is in the form Fe3O4. If a 2.0-ton sample of taconite pellets yields 1075 pounds of iron when it is refined, what is the mass percentage of Fe3O4 in taconite?
The characteristic odor of decaying flesh is due to the presence of various nitrogen-containing compounds. One such compound, called putrescine, was analyzed and found to contain 54.49% carbon, 13.72% hydrogen, and 31.78% nitrogen by mass. If the molar mass of putrescine is known to be between 85
Iron–platinum alloys may be useful as high-density recording materials because of their magnetic properties. These alloys have been made with a wide range of composition, from 34.0 at% Pt to 81.8 at% Pt. Express this range in mol%.
Some aluminum–lithium alloys display the property of superplasticity, meaning they can undergo tensile deformation by large amounts (1000 times or more) without breaking. If such an alloy has 4 wt% Li, what is its composition in mol%? Explain the relative magnitudes of the mole percentage and
Classify the following compounds as acids or bases, weak or strong.(a) Perchloric acid, (b) Cesium hydroxide,(c) Carbonic acid, H2CO3, (d) Ethylamine, C2H5NH2
Nitric acid is often sold and transported as a concentrated 16 M aqueous solution. How many gallons of such a solution would be needed to contain the roughly 2.1 × 109 pounds of HNO3 produced annually in the United States?
Twenty-five mL of a 0.388 M solution of Na2SO4 is mixed with 35.3 mL of 0.229 M Na2SO4. What is the molarity of the resulting solution? Assume that the volumes are additive.
As computer processor speeds increase, it is necessary for engineers to increase the number of circuit elements packed into a given area. Individual circuit elements are often connected using very small copper “wires” deposited directly onto the surface of the chip. In some processors, these
As chip speeds increase, the width of the interconnects described in Problem 3.107 must be reduced. A hypothetical limit to this process would be reached if the interconnect was just one copper atom wide. Use the density of copper (8.96 g/cm3) to estimate the diameter of a copper atom. (Optical
Materials engineers often create new alloys in an effort to improve the properties of an existing material. ZnO based semiconductors show promise in applications like light-emitting diodes, but their performance can be enhanced by the addition of small amounts of cadmium.One material that has been
The protein that carries oxygen in the blood is called hemoglobin. It is 0.335% Fe by mass. Given that a molecule of hemoglobin contains four iron atoms, describe how you can calculate the molar mass of hemoglobin. Do you need to look up anything to do it?
The chlorophyll molecule responsible for photosynthesis in plants contains 2.72% Mg by mass. There is only one Mg atom per chlorophyll molecule. How can you determine the molar mass of chlorophyll based on this information?
In one experiment, the burning of 0.614 g of sulfur produced 1.246 g of sulfur dioxide as its only product. In a second experiment run to verify the outcome of the first, a sample was burned, and 0.813 g of sulfur dioxide was obtained, but the student running the experiment forgot to determine the
MgCl2 is often found as an impurity in table salt (NaCl). If a 0.05200-g sample of table salt is found to contain 61.10% Cl by mass, describe how you could determine the percentage of MgCl2 in the sample.
Under the Clean Air Act, companies can purchase the right to emit certain pollutants from other companies that emit less than they are allowed by law. Suppose that the cost to purchase a pollution credit for 1 ton of sulfur dioxide is $300. Describe how you would determine how many SO2 molecules
The average person exhales 1.0 kg of carbon dioxide in a day. Describe how you would estimate the number of CO2 molecules exhaled per breath for this average person.
Biomass production and use is a small component in the increase of CO2 in the atmosphere. (a) What is the main source of CO2 increase in the atmosphere?(b) In what way is this source similar to the use of biomass fuels?
What is meant by the term carbon reservoir? What are the two largest carbon reservoirs for our planet?
What is meant by the term carbon sequestration?
Explain how the burning of fossil fuels, which contributes only 7.0 Pg yr–1 to the atmospheric store of carbon, can upset the balance of carbon in the atmosphere if photosynthesis fixes 120 Pg yr–1.
Are most proposals to carry out carbon sequestration based on chemical or physical properties of CO2? Defend your answer.
The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone
Answer each of the following questions. That none of them should require difficult calculations.(a) How many molecules are present in 1 mole of octane (C8H18)?(b) How many moles of fluorine atoms are present in 4 moles of C2F6?(c) What is the approximate mass (to the nearest gram) of 3 × 1023
Consider two samples of liquid: 1 mole of water (H2O) and 1 mole of ethanol (C2H5OH). Answer each of the following questions. Note that none of these should require significant calculations.(a) Which sample contains more atoms?(b) Which sample contains more molecules?(c) Which sample has a larger
The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place.(b) Write a balanced chemical equation for the reaction, using the smallest possible
Consider two samples. Sample A contains 2 moles of N2 and 1 mole of O2, and Sample B contains 1 mole of N2O5.(a) Which sample contains more molecules?(b) Which sample contains more oxygen atoms?(c) Which sample contains more nitrogen atoms?
Which one of the following metal samples cannot possibly exist? Why not?(a) A piece of gold foil 10–6 m thick (b) 5 mg of platinum(c) 10–24 mol of aluminum(d) A copper wire 0.1 mm in diameter
The particulate scale drawing shown depicts the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place.(b) Write a balanced chemical equation for the reaction, using the smallest possible
Tetraphosphorus trisulfide, P4S3, is used in the manufacture of “strike anywhere” matches. Elemental phosphorus and sulfur react directly to form P4S3:If we have 153 g of S8 and an excess of phosphorus, what mass of P4S3 can be produced by this reaction?Strategy The heart of any stoichiometry
Explain the difference between complete and incomplete combustion.
The simplest approximate chemical formula for the human body could be written as C728H4850O1970N104Ca24P16 K4S4Na3Cl2Mg. Based on this formula, describe how you would rank by mass the ten most abundant elements in the human body.
For the oxides of iron, FeO, Fe2O3, and Fe3O4, describe how you would determine which has the greatest percentage by mass of oxygen. Would you need to look up any information to solve this problem?
Consider common sugars such as glucose (C6H12O6) and sucrose (C12H22O11). What type of chemical bonding would you expect to find in these chemicals?
For the compounds that commonly undergo precipitation reactions, what type of chemical bonding is expected?
If you have 32.6 g of sodium carbonate that is dissolved to give 2.10 L of solution, what is the molarity of the solution? What is the molarity of the sodium ions?
If you have 21.1 g of iron (II) nitrate that is dissolved to give 1.54 L of solution, what is the molarity of the solution? What is the molarity of the nitrate ions?
What type of reasoning were we using when we developed the equation for dilution, Mi × Vi = Mf × Vf?
Most periodic tables provide molar masses with four or five significant figures for the elements. How accurately would you have to measure the mass of a sample of roughly 100 g to make a calculation of the number of moles of the chemical to have its significant figures limited by the molar mass
In the combustion of methane, how many moles of O2 are required if 6.75 mol of CH4 is to be completely consumed?Strategy We start with the balanced chemical equation and use the stoichiometric coefficients to establish the mole ratio between methane and oxygen. Then, we can use that ratio to relate
List at least two factors that make it difficult to describe the combustion of gasoline accurately. What assumptions can be made to address these complications?
What is an alkane?
Based on what you’ve learned in this chapter, would you classify the chemistry of polymers as organic or inorganic?Why?
How can an element have an atomic weight that is not an integer?
Explain the concept of a “weighted” average in your own words.
The accompanying table provides the identity of the two naturally occurring isotopes for four elements and the atomic weights for those elements. (In each case, the two isotopes differ in mass number by two.) Which element has the mass spectrum shown? Explain your answer. Isotopes 121 Sb, 123
In general, how are electrons involved in chemical bonding?
Conduction of electricity usually involves the movement of electrons. Based on the concept of metallic bonding, explain why metals are good conductors of electricity.
Describe how a covalently bonded molecule is different from compounds that are either ionic or metallic.
Of the following elements, which two would you expect to exhibit the greatest similarity in physical and chemical properties? Cl, P, S, Se, Ti. Explain your choice.
How do binary compounds with hydrogen illustrate the concept of periodicity?
Which binary combinations of elements are most likely to give ionic substances?
Why are there different rules for naming covalent and ionic binary compounds?
Early attempts to arrange the elements often focused on atomic weight. Mendeleev considered a number of properties in addition to atomic weight, so he realized that some elements seemed out of place when ordered by atomic weight. Using the modern periodic table, identify elements for which
Describe how the saying “opposites attract” corresponds with the mathematical representation of Coulomb’s law shown in Equation 2.1. Remember that attractive forces have negative values and repulsive forces have positive values.Equation 2.1 9192 4π²01² F=- (2.1)
For some uses, the relative abundance of isotopes must be manipulated. For example, a medical technique called boron neutron capture therapy needs a higher fraction of 10B than occurs naturally to achieve its best efficiency.What would happen to the atomic weight of a sample of boron that had been
What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must be true about the nuclei of atoms with higher atomic numbers?
Describe how you can identify the isotope, X, in this puzzle.The nucleus contains one more neutron than proton, and the mass number is nine times larger than the charge on the ion X3+.
Many transition metals produce more than one ion. For example, iron has ions with charges of 2+ and 3+ that are both common. How could you use the compounds of a transition metal with oxygen to determine the charge of the metal ion? Use iron as your example.
Naturally occurring europium has an average atomic weight of 151.964 amu. If the only isotopes of europium present are 151Eu and 153Eu, describe how you would determine the relative abundance of the two isotopes. Include in your description any information that would need to be looked up.
A candy manufacturer makes chocolate-covered cherries. Although all of the products look roughly the same, 3% of them are missing the cherry. The mass of the candy with a cherry is 18.5 g; those missing the cherry weigh only 6.4 g.
Two common oxides of iron are FeO and Fe2O3. Based on this information, tell how you would predict two common compounds of iron and chlorine.
Use a molecular level description to distinguish betweenLDPE and HDPE.
Engineers who design bicycle frames are familiar with the densities of aluminum (2.699 g/cm3), steel (7.87 g/cm3), and titanium (4.507 g/cm3). How does this information compare with Figure 2.12, and what would it suggest for changes in this figure if more shades were used for the density
Are the elements designated as critical materials all rare? Explain your answer.
In what country is most of the world’s cobalt mined? What events in that country dramatically affected the price of cobalt?
In what types of technology do the elements designated as critical materials generally play important roles?
Based on the information in Figure 1.1, which three elements would you argue are the most critical among the “critical materials”? Justify your answer.Figure 1.1 to clean energy Importance (high) 3 2 1 (low) Nickel 1 (low) Critical Lithium Tellurium m Samarium 2 Neodymium
The mass density of water at 25°C is 0.997 g per mL. A child’s swimming pool holds 346 L of water at this temperature. What mass of water is in the pool?Strategy We want to use the density as a ratio, but first we must express the volume in appropriate units. We can convert the volume of the
In what region of the periodic table are most of the elements that are listed as critical materials found?
What agency of the U.S. government is responsible for identifying an element as a critical material? What sorts of applications are the primary concern of this agency?
Dry ice is solid carbon dioxide; it is called “dry” because it goes directly from a solid to a gas without becoming a liquid under ordinary conditions. Draw a picture that shows what the carbon dioxide molecules might look like as a solid and as a gas.Strategy To answer conceptual questions
When we make observations in the laboratory, which perspective of chemistry are we normally using?

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