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engineering
chemical engineering

Chemical Principles 7th edition Steven S. Zumdahl, Donald J. DeCoste - Solutions

Silver sulfadiazine burn- treating cream creates a barrier against bacterial invasion and releases antimicrobial agents directly into the wound. If 25.0 g of Ag2O is reacted with 50.0 g of C10H10N4SO2, what mass of silver sulfadiazine (AgC10H9N4SO2) can be produced, assuming 100% yield?Ag2O(s) +
Bornite (Cu3FeS3) is a copper ore used in the production of copper. When heated, the following reaction occurs:2Cu3FeS3(s) + 7O2(g) → 6Cu(s) + 2FeO(s) + 6SO2(g)If 2.50 metric tons of bornite is reacted with excess O2 and the process has an 86.3% yield of copper, how much copper is produced?
DDT, an insecticide harmful to fish, birds, and humans, is produced by the following reaction: 2C6H5Cl + C2HOCl3 → C14H9Cl5 + H2OChlorobenzene Chloral DDT In a government lab, 1142 g of chlorobenzene is reacted with 485 g of chloral.a. What mass of DDT is formed, assuming 100% yield?b. Which
Hydrogen cyanide is produced industrially from the reaction of gaseous ammonia, oxygen, and methane:2NH3(g) + 3O2(g) + 2CH4(g) → 2HCN( g) + 6H2O(g)If 5.00 × 103 kg each of NH3, O2, and CH4 are reacted, what mass of HCN and of H2O will be produced, assuming 100% yield?
An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass 205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass 207.9766 amu. Calculate the average atomic mass and identify the element.
The production capacity for acrylonitrile (C3H3N) in the United States exceeds 2 million pounds per year. Acrylo-nitrile, the building block for polyacrylonitrile fibers and a variety of plastics, is produced from gaseous propylene, ammonia, and oxygen:2C3H6(g) + 2NH3(g) + 3O2(g) → 2C3H3N(g) +
Consider the following unbalanced reaction:P4(s) + F2(g) → PF3(g)How many grams of F2 are needed to produce 120g of PF3 if the reaction has a 78.1% yield?
The aspirin substitute acetaminophen (C8H9O2N) is produced by the following three-step synthesis:I. C6H5O3N(s) + 3H2(g) + HCl(aq) → C6H8ONCl(s) + 2H2O(l)II. C6H8ONCl(s) + NaOH(aq) → C6H7ON(s) + H2O(l) + NaCl(aq)III. C6H7ON(s) + C4H6O3(l) →C8H9O2N(s) + HC2H3O2(l)The first two reactions have
A sample of a hydrocarbon (a compound consisting of only carbon and hydrogen) contains 2.59 × 1023 atoms of hydrogen and is 17.3% hydrogen by mass. If the molar mass of the hydrocarbon is between 55 and 65 g/mol, how many moles of compound are present, and what is the mass of the sample?
A binary compound created by the reaction of an un-known element E and hydrogen contains 91.27% E and 8.73% H by mass. If the formula of the compound is E3H8, calculate the atomic mass of E.
An ionic compound MX3 is prepared according to the following unbalanced chemical equation: M + X2 → MX3 A 0.105g sample of X2 contains 8.92 × 1020 molecules. The compound MX3 consists of 54.47% X by mass. What are the identities of M and X, and what is the correct name for MX3? Starting with
The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol. How many H atoms are present in a 2.00-g sample of styrene?
A 0.755-g sample of hydrated copper(II) sulfate (CuSO4 ? xH2O) was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO4) with a mass of 0.483 g. Determine the value of x. [This number is called the “ number of waters of hydration” of copper(II) sulfate. It
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000 kg/h. How much water must be evaporated per hour if the final product contains only 20% water?
When aluminum metal is heated with an element from Group 6A of the periodic table, an ionic compound forms. When the experiment is performed with an unknown Group 6A element, the product is 18.56% Al by mass. What is the formula of the compound?
The mass spectrum of bromine (Br2) consists of three peaks with the following relative sizes: Mass (amu) Relative Size 157.84.................................................... 0.2534 159.84...................................................
A salt contains only barium and one of the halide ions. A 0.158-g sample of the salt was dissolved in water, and an excess of sulfuric acid was added to form barium sulfate (BaSO4), which was filtered, dried, and weighed. Its mass was found to be 0.124 g. What is the formula of the barium halide?
A sample of LSD (d- lysergic acid diethylamide, C24H30N3O) is added to some table salt (sodium chloride) to form a mixture. Given that a 1.00- g sample of the mixture undergoes combustion to produce 1.20 g of CO2, what is the mass percentage of LSD in the mixture?
Consider the following unbalanced equation:Ca3(PO4) 2(s) + H2SO4(aq) → CaSO4(s) + H3PO4(aq)What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg of calcium phosphate with 1.0 kg of concentrated sulfuric acid (98% H2SO4 by mass)?
A 0.4230g sample of impure sodium nitrate was heated, converting all the sodium nitrate to 0.2864 g of sodium nitrite and oxygen gas. Determine the percent of sodium nitrate in the original sample.
You have seven closed containers, each with equal masses of chlorine gas (Cl2). You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation
An iron ore sample contains Fe2O3 plus other impurities. A 752- g sample of impure iron ore is heated with excess carbon, producing 453 g of pure iron by the following reaction:Fe2O3(s) + 3C(s) → 2Fe(s) + 3CO(g)What is the mass percent of Fe2O3 in the impure iron ore sample? Assume that
In using a mass spectrometer, a chemist sees a peak at a mass of 30.0106. Of the choices 12C2 1H6, 12C1H2 16O, and 14N16O, which is responsible for this peak? Pertinent masses are 1H, 1.007825; 16O, 15.994915; and 14N, 14.003074.
Natural rubidium has the average mass 85.4678 amu and is composed of isotopes 85Rb (mass 5 84.9117 amu) and 87Rb. The ratio of atoms 85Rb/ 87Rb in natural rubidium is 2.591. Calculate the mass of 87Rb.
Tetrodotoxin is a toxic chemical found in fugu pufferfish, a popular but rare delicacy in Japan. This compound has an LD50 (the amount of substance that is lethal to 50% of a population sample) of 10 mg per kg of body mass. Tetrodotoxin is 41.38% carbon by mass, 13.16% nitrogen by mass, and 5.37%
Consider the following data for three binary compounds of hydrogen and nitrogen:When 1.00 L of each gaseous compound is decomposed to its elements, the following volumes of H2(g) and N2(g) are obtained:Use these data to determine the molecular formulas of compounds I, II, and III and to determine
Naturally occurring tellurium (Te) has the following isotopic abundances:
A 0.200- g sample of protactinium(IV) oxide is converted to another oxide of protactinium by heating in the presence of oxygen to give 0.2081 g of the new oxide, PaxOy. Determine the values of x and y.
A 1.000- g sample of XI2 is dissolved in water, and excess silver nitrate is added to precipitate all of the iodide as AgI. The mass of the dry AgI is found to be 1.375 g. Calculate the atomic weight (mass) of X.
A substance X2Z has the composition (by mass) of 40.0% X and 60.0% Z. What is the composition (by mass) of the compound XZ2?
Vitamin A has a molar mass of 286.4 g and has a general molecular formula of CxHyE, where E is an un-known element. If vitamin A is 83.86% C and 10.56% H by mass, what is the molecular formula of vitamin A?
Boron consists of two isotopes, 10B and 11B. Chlorine also has two isotopes, 35Cl and 37Cl. Consider the mass spectrum of BCl3. How many peaks would be present, and what approximate mass would each peak correspond to in the BCl3 mass spectrum?
In a mass spectrometer, positive ions are produced when a gaseous mixture is ionized by electron bombardment produced by an electric discharge. When the electric-discharge voltage is low, singly positive ions are produced and the following peaks are observed in the mass spectrum:Mass (amu) Relative
When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of FeO and Fe2O3. In a certain experiment, 20.00 g of iron metal was reacted with 11.20 g of oxygen gas. After the experiment, the iron was totally consumed and 3.24 g of oxygen gas remained. Calculate the
Element X forms both a dichloride (XCl2) and a tetra-chloride (XCl4). Treatment of 10.00 g of XCl2 with excess chlorine forms 12.55 g of XCl4. Calculate the atomic weight (mass) of X and identify X.
Zinc and magnesium metal each react with hydrochloric acid to make chloride salts of the respective metals and hydrogen gas. A 10.00- g mixture of zinc and magnesium produces 0.5171 g of hydrogen gas upon being mixed with an excess of hydrochloric acid. Determine the percent magnesium by mass in
An unknown binary compound containing hydrogen (XHn) has a density as a gas that is 2.393 times that of oxygen gas under the same conditions. When 2.23 × 10-2 mole of this compound reacts with excess oxygen gas, 0.803 g of water is produced. Identify the element X in this compound.
Gallium arsenide (GaAs) has gained widespread use in semiconductor devices that interconvert light and electrical signals in fiber-optic communications systems. Gallium consists of 60.% 69Ga and 40.% 71Ga. Arsenic has only one naturally occurring isotope, 75As. Gallium arsenide is a polymeric
A 2.25-g sample of scandium metal is reacted with excess hydrochloric acid to produce 0.1502 g hydrogen gas. What is the formula of the scandium chloride produced in the reaction?
When M2S3(s) is heated in air, it is converted to MO2(s). A 4.000- g sample of M2S3(s) shows a decrease in mass of 0.277 g when it is heated in air. What is the average atomic mass of M?
Consider a gaseous binary compound with a molar mass of 62.09 g/mol. When 1.39 g of this compound is completely burned in excess oxygen, 1.21 g of water is formed. Determine the formula of the compound.
Pure carbon was burned in an excess of oxygen. The gaseous products were CO2 72.0 mol% CO 16.0 mol% O2 12.0 mol% How many moles of O2 were present in the initial reaction mixture for every mole of carbon?
You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/ mol. Reacting 1 mole of salicylic acid with 1 mole of acetic anhydride
Lanthanum was reacted with hydrogen in a given experiment to produce the nonstoichiometric compound LaH2.90. Assuming that the compound contains H2, La2+, and La3+, calculate the fraction of La2+and La3+ present.
A 9.780-g gaseous mixture contains ethane (C2H6) and propane (C3H8). Complete combustion to form carbon dioxide and water requires 1.120 moles of oxygen gas. Calculate the mass percent of ethane in the original mixture.
Consider a mixture of potassium chloride and potassium nitrate that is 43.2% potassium by mass. What is the percent KCl by mass of the original mixture?
A 2.077 g sample of an element, which has an atomic mass between 40 and 55, reacts with oxygen to form 3.708 g of an oxide. Determine the formula of the oxide and identify the element.
Ammonia reacts with O2 to form either NO(g) or NO2(g) according to these unbalanced equations: NH3(g) + O2(g) → NO(g) + H2O(g) NH3(g) + O2(g) → NO2(g) + H2O(g) In a certain experiment, 2.00 moles of NH3(g) and 10.00 moles of O2(g) are contained in a closed flask. After the reaction is complete,
What is electrochemistry? What are redox reactions? Explain the difference between a galvanic cell and an electrolytic cell.
Given the following two standard reduction potentials, M3+ + 3e– → M ϐo = 20.10 VM2+ + 2e– → M ϐo = 20.50 V determine for the standard reduction potential of the half reaction M3+ + e– → M2+ (You must use the extensive property ΔGo to determine the standard reduction
Zirconium is one of the few metals that retains its structural integrity upon exposure to radiation. For this reason, the fuel rods in most nuclear reactors are made of zirconium. Answer the following questions about the redox properties of zirconium based on the half reaction ZrO2 ? H2O + H2O
A galvanic cell is based on the following half reactions:Cu2+ + 2e- → Cu(s) ϐo = 0.34 VV2+ + 2e- → V(s) ϐo = 21.20 VIn this cell the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown
Answer the following questions using data from Table (all under standard conditions).a. Is H+(aq) capable of oxidizing Cu(s) to Cu2+(aq)?b. Is Fe3+(aq) capable of oxidizing I2(aq)?c. Is H2(g) capable of reducing Ag+(aq)?d. Is Fe2+(aq) capable of reducing Cr3+(aq) to Cr2+(aq)?Table
Using data from Table, place the following in order of increasing strength as oxidizing agents (all under standard conditions). Cd2+, IO3-, K1, H2O, AuCl4-, and I2Table
Using data from Table, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+, F2, H2, H2O, I2, and KTable
Consider only the species (at standard conditions) Br2, Br2, H+, H2, La3+, Ca, Cd in answering the following questions. Give reasons for your answers.a. Which is the strongest oxidizing agent?b. Which is the strongest reducing agent?c. Which species can be oxidized by MnO4- in acid? d. Which
A patent attorney has asked for your advice concerning the merits of a patent application claiming the invention of an aqueous single galvanic cell capable of producing a 12 V potential. Comment.
The free energy change for a reaction ΔG is an extensive property. What is an extensive property? Surprisingly, one can calculate ΔG from the cell potential for the reaction. This is surprising because is an intensive property. How can the extensive property ΔG be calculated from the intensive
When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg
Estimate E°cell for the half reaction. 2H2O + 2e- → H2 + 2OH- given the following values of ΔGof :H2O(l) = –237 kJ/ mol H2(g) = 0.0 OH-(aq) = –157 kJ/ mol e- = 0.0 Compare this value of E°cell with the value of E°cell given in Table.Table
Glucose is the major fuel for most living cells. The oxidative breakdown of glucose by our body to produce energy is called respiration. The reaction for the complete combustion of glucose is C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)If this combustion reaction could be harnessed as
Calculate the maximum amount of work that can be obtained from the galvanic cells at standard conditions in Exercise 22.Galvanic Cell in exercise 22.Consider the following galvanic cells:
Under standard conditions, what reaction occurs, if any, when each of the following operations are performed?a. Crystals of I2 are added to a solution of NaCl.b. Cl2 gas is bubbled into a solution of NaI.c. A silver wire is placed in a solution of CuCl2.d. An acidic solution of FeSO4 is exposed to
Calculate ΔGo and K at 25oC for the galvanic cell reactions in Exercise 21.Reactions in exercise 21. a. Cl2 + 2e- → 2Cl2 E°cell = 1.36 VBr2 + 2e- → 2Br2 E°cell = 1.09 Vb. MnO4- + 8H+ + 5e- → Mn2+ + 4H2O E°cell = 1.51 VIO4- + 2H+ + 2e- →
Chlorine dioxide (ClO2), which is produced by the reaction2NaClO2(aq) + Cl2(g) → 2ClO2(g) + 2NaCl(aq)has been tested as a disinfectant for municipal water treatment.a. Using data from Table 11.1, calculate ϐo, ΔGo, and K at 25oC for the production of ClO2.b. One of the concerns in
The overall reaction and equilibrium constant value for a hydrogen–oxygen fuel cell at 298 K is 2H2(g) + O2(g) → 2H2O(l) K = 1.28 × 1083a. Calculate E°cell and ΔG8 at 298 K for the fuel cell reaction.b. Predict the signs of ΔHo and ΔSo for the fuel cell reaction.c. As
Consider the following galvanic cell:a. Label the reducing agent and the oxidizing agent, and describe the direction of the electron flow.b. Determine the standard cell potential.c. Which electrode increases in mass as the reaction proceeds and which electrode decreases in mass?
Calculate E°cell for the reactionCH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) Using values of ΔGof in Appendix 4. Will E°cell increase or decrease with an increase in temperature?
A disproportionation reaction involves a substance that acts as both an oxidizing agent and a reducing agent, producing higher and lower oxidation states of the same element in the products. Which of the following disproportionation reactions are spontaneous under standard conditions? Calculate
Calculate E°cell for the following half reaction:AgI(s) + e- → Ag(s) + I2Reference the Ksp value for AgI and the standard reduction potential for Ag+.
For the following half reaction, E°cell = 22.07 V:AlF63– + 3e- → Al + 6F2Using data from Table 11.1, calculate the equilibrium constant at 25oC for the reaction Al3+(aq) 1 6F2(aq) ⇌ AlF63–(aq)Table 11.1
Calculate Ksp for iron(II) sulfide given the following data:
CuI + e€“ †’ Cu + I2
2Al(s) + Cr2O72€“(aq) + 14H+(aq) †’ 2Al3+(aq) + 2Cr3+(aq) + 7H2O(l)
Consider the galvanic cell based on the following halfreactions:b. Calculate Î”Go and K for the cell reaction at 25oC. c. Calculate cell at 25oC when [Zn2+] = 0.10 M and [Fe2+] = 1.0 Ã— 10€“5 M.
Consider the galvanic cell based on the following halfreactions:b. Calculate Î”Go and K for the cell reaction at 25oC. c. Calculate cell at 25oC when [Au3+] = 1.0 Ã— 10€“2 M and [Tl+] = 1.0 Ã— 10€“4 M.
How can you construct a galvanic cell from two substances, each having a negative standard reduction potential?
Consider the following galvanic cell at 25oC: Pt | Cr2+ (0.30 M), Cr3+(2.0 M) | | Co2+(0.20 M) | Co The overall reaction and equilibrium constant value are 2Cr2+(aq) + Co2+(aq) → 2Cr3+(aq) + Co(s) K = 2.79 × 107 Calculate the cell potential ϐ for this galvanic cell and ΔG for the cell
Consider the cell described below: Al | Al3+(1.00 M) | | Pb2+ (1.00 M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al3+] to have changed by 0.60 mol/ L. (Assume T = 25oC.)
The Nernst equation can be applied to half reactions. Calculate the reduction potential at 25oC of each of the following half cells. a. Cu/ Cu2+ (0.10 M) (The half reaction is Cu2+ + 2e– n Cu.) b. Cu/ Cu2+ (2.0 M) c. Cu/ Cu2+(1.0 × 10–4 M) d. MnO4– (0.10 M)/ Mn2+ (0.010 M) at pH = 3.00 (The
The overall reaction in the lead storage battery isPb(s) + PbO2(s) + 2H+(aq) + 2HSO4-(aq) †’ 2PbSO4(s) + 2H2O(l)d. Based on your previous answers, why does it seem that batteries fail more often on cold days than on warm days?
A chemist wishes to determine the concentration of CrO42- electrochemically. A cell is constructed consisting of a saturated calomel electrode (SCE; see Exercise 24) and a silver wire coated with Ag2CrO4. The E° value for the following half reaction is 10.446 V relative to the standard hydrogen
A silver concentration cell is set up at 25oC as shown below:The AgCl(s) is in excess in the left compartment. a. Label the anode and cathode, and describe the direction of the electron flow. b. Determine the value of Ksp for AgCl at 25oC.
Consider the concentration cell shown below. Calculate the cell potential at 25oC when the concentration of Ni2+ in the compartment on the right has each of the following values.a. 1.0 M b. 2.0 M
An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25oC if the copper electrode is placed in a solution in which [Cu2+] = 2.5 × 1024 M?b. If the copper electrode is placed in a solution of 0.10 M NaOH that is
Sketch the galvanic cells based on the following overall reactions. Calculate ϐo, show the direction of electron flow and the direction of ion migration through the salt bridge, identify the cathode and anode, and give the overall balanced equation. Assume that all concentrations are 1.0 M and
You have a concentration cell in which the cathode has a silver electrode with 0.10 M Ag+. The anode also has a silver electrode with Ag+(aq), 0.050 M S2O32–, and 1.0 × 1023 M Ag(S2O3)23–. You read the voltage to be 0.76 V.a. Calculate the concentration of Ag+ at the anode.b. Determine the
Consider a galvanic cell at standard conditions based on the following half reactions:Au3+ + 3e- → Au ϐo = 1.50 VFe3+ + e- → Fe2+ ϐo = 0.77 VWhen enough NaCl(s) is added to the compartment containing gold to make the [Cl2] = 0.10 M, the cell potential is observed to be 0.31 V. Assume that
How long will it take to plate out each of the following with a current of 100.0 A?a. 1.0 kg of Al from aqueous Al3+b. 1.0 g of Ni from aqueous Ni2+c. 5.0 moles of Ag from aqueous Ag+
What mass of each of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from aqueous Co2+c. I2 from aqueous KIb. Hf from aqueous Hf4+d. Cr from molten CrO3
Why is the electrolysis of molten salts much easier to predict in terms of what occurs at the anode and cathode than the electrolysis of aqueous dissolved salts?
What reactions take place at the cathode and the anode when each of the following is electrolyzed? Assume standard conditions.a. Molten NiBr2b. Molten AlF3c. Molten MnI2
Calculate E°cell values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations. Standard reduction potentials are found in Table 11.1. a. MnO4-(aq) + I2(aq) ⇌ I2(aq) + Mn2+(aq)b. MnO4-(aq) +
Consider the following half reactions: IrCl63– + 3e- → Ir 1 6Cl2 ϐo = 0.77 V PtCl42- + 2e- → Pt 1 4Cl2 ϐo = 0.73 V PdCl42– + 2e– → Pd 1 4Cl2 ϐo = 0.62 V
Electrolysis of an alkaline earth metal chloride using a current of 5.00 A for 748 seconds deposits 0.471 g of metal at the cathode. What is the identity of the alkaline earth metal chloride?
One of the few industrial scale processes that produces organic compounds electrochemically is used by the Monsanto Company to produce 1,4 dicyanobutane. The reduction reaction is 2CH2PCHCN + 2H+ + 2e– → NCO(CH2)4OCN The NCO(CH2)4OCN is then chemically reduced by hydrogen to H2NO(CH2)6ONH2,
What volume of F2 gas, at 25oC and 1.00 atm, is produced when molten KF is electrolyzed by a current of 10.0 A for 2.00 h? What mass of potassium metal is produced? At which electrode does each reaction occur?
It takes 15 kWh (kilowatt hours) of electrical energy to produce 1.0 kg of aluminum metal from aluminum oxide by the Hall–Heroult process. Compare this value with the amount of energy necessary to melt 1.0 kg of aluminum metal. Why is it economically feasible to recycle aluminum cans? (The
Sketch the galvanic cells based on the following half-reactions. Calculate Ïo, show the direction of electron flow and the direction of ion migration through the salt bridge, identify the cathode and anode, and give the overall balanced equation. Assume that all concentrations are 1.0 M
What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of 2.50 A in 15.0 min?

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