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engineering
the science and engineering of materials

Chemistry 10th Edition Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste - Solutions

When 6 M ammonia is added gradually to aqueous copper(II) nitrate, a white precipitate forms. The precipitate dissolves as more 6 M ammonia is added. Write balanced equations to explain these observations.
When an aqueous solution of KCN is added to a solution containing Ni2+ ions, a precipitate forms, which redissolves on addition of more KCN solution. Write reactions describing what happens in this solution.
Consider aqueous solutions of the following coordination compounds: [Cr(NH3)3Cl3], [Cr(NH3)6]Cl3, Na3[CrCl6]. If silver nitrate is added to each solution, in which will a precipitate form? Explain.
A coordination compound of cobalt(III) contains four ammonia molecules, one sulfate ion, and one chloride ion. Addition of aqueous BaCl2 solution to an aqueous solution of the compound gives no precipitate. Addition of aqueous AgNO3 to an aqueous solution of the compound produces a white
Draw all geometrical and linkage isomers of square planar Pt(NH3)2(SCN)2.
What roles do kinetics and thermodynamics play in the effect that the following reaction has on the properties of steel? 3Fe + C Fe3C
The CrF64- ion is known to have four unpaired electrons. Does the F- ligand produce a strong or weak field?
Silver is sometimes found in nature as large nuggets; more often it is found mixed with other metals and their ores. Cyanide ion is often used to extract the silver by the following reaction that occurs in basic solution:Balance this equation by using the half-reaction method. Ag(s) + CN¯(aq) +
The complex ion NiCl42- has two unpaired electrons, whereas Ni(CN)42- is diamagnetic. Propose structures for these two complex ions.
How many unpaired electrons are present in the tetrahedral ion FeCl4-?
The following statements discuss some coordination compounds. For each coordination compound, give the complex ion and the counterions, the electron configuration of the transition metal, and the geometry of the complex ion.a. CoCl2 ? 6H2O is a compound used in novelty devices that predict
For the process what would be the expected ratio of cis to trans isomers in the product? Co(NH3),C1²+ (aq) + Cl¯(aq) Co(NH3)4Cl₂+ (aq) + NH3(aq)
Name the following coordination compounds.a. Na4[Ni(C2O4)3]b. K2[CoCl4]c. [Cu(NH3)4]SO4d. [Co(en)2(SCN)Cl]Cl
In which of the following is(are) the electron configuration(s) correct for the species indicated? a. Cu [Ar]4s2 3d9b. Fe3+ [Ar]3d5c. Co [Ar]4s2 3d7d. La [Ar]6s2 4f1e. Pt2+ [Xe]4f145d8
The following table indicates the number of unpaired electrons in the crystal field diagrams for some complexes. Complete the table by classifying each species as weak field, strong field, or insufficient information. Unpaired Species Electrons
Which of the following ions is(are) expected to form colored octahedral aqueous complex ions? a. Zn2+b. Cu2+c. Mn3+d. Ti4+
Will 0.10 mol of AgBr completely dissolve in 1.0 L of 3.0 M NH3? The Ksp value for AgBr(s) is 5.0 × 10-13, and the overall formation constant for the complex ion Ag(NH3)2+ is 1.7 × 107 , that is, Ag (aq) + 2NH3(aq) Ag(NH3)2 (aq) K = 1.7 x 107
Ammonia and potassium iodide solutions are added to an aqueous solution of Cr(NO3)3. A solid is isolated (compound A), and the following data are collected:i. When 0.105 g of compound A was strongly heated in excess O2, 0.0203 g CrO3 was formed.ii. In a second experiment it took 32.93 mL of 0.100 M
There are three salts that contain complex ions of chromium and have the molecular formula CrCl3 ? 6H2O. Treating 0.27 g of the first salt with a strong dehydrating agent resulted in a mass loss of 0.036 g. Treating 270 mg of the second salt with the same dehydrating agent resulted in a mass loss
Define fission and fusion. How does the energy associated with fission or fusion processes compare to the energy changes associated with chemical reactions? Fusion processes are more likely to occur for lighter elements, whereas fission processes are more likely to occur for heavier elements. Why?
Three electrochemical cells were connected in series so that the same quantity of electrical current passes through all three cells. In the first cell, 1.15 g chromium metal was deposited from a chromium(III) nitrate solution. In the second cell, 3.15 g osmium was deposited from a solution made of
Gas A2 reacts with gas B2 to form gas AB at a constant temperature. The bond energy of AB is much greater than that of either reactant. What can be said about the sign of ΔH? ΔSsurr? ΔS? Explain how potential energy changes for this process. Explain how random kinetic energy changes during the
Calculate ΔGο and K at 25οC for the reactions in Exercises 38 and 42.Data in Exercises 38:Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the
What characterizes an electrolytic cell? What is an ampere? When the current applied to an electrolytic cell is multiplied by the time in seconds, what quantity is determined? How is this quantity converted to moles of electrons required? How are moles of electrons required converted to moles of
What type of radioactive decay must occur for each of the following nuclear processes? a. Process 1b. Process 2c. Process 3 Mass number 214 210 206 202 198 3 O 79 80 81 82 83 84 Atomic number
All radioactive decay processes follow first-order kinetics. What does this mean? What happens to the rate of radioactive decay as the number of nuclides is halved? Write the first-order rate law and the integrated firstorder rate law. Define the terms in each equation. What is the half-life
Do radiotracers generally have long or short half-lives? Explain.
What is a nuclear transformation? How do you balance nuclear transformation reactions? Particle accelerators are used to perform nuclear transformations. What is a particle accelerator?
What are transuranium elements and how are they synthesized?
The fission of uranium-235 is used exclusively in nuclear power plants located in the United States. There are many different fission reactions of uranium-235, but all the fission reactions are self-sustaining chain reactions. Explain. Differentiate between the terms critical, subcritical, and
Why are the observed energy changes for nuclear processes so much larger than the energy changes for chemical and physical processes?
Describe the relative penetrating powers of alpha, beta, and gamma radiation.
Explain the difference between somatic damage from radiation and genetic damage. Which type causes immediate damage to the exposed individual?
A recent study concluded that any amount of radiation exposure can cause biological damage. Explain the differences between the two models of radiation damage, the linear model and the threshold model.
Thorium-232 is known to undergo a progressive decay series until it reaches stability at lead-208. For each step of the series indicated in the table below, which nuclear particle is emitted? Parent Nuclide Particle
The radioactive isotope 242Cm decays by a series of α-particle and β-particle productions, taking 242Cm through many transformations to end up as 206Pb. In the complete decay series, how many α and β particles are produced?
The stable isotopes of boron are boron-10 and boron-11. Four radioactive isotopes with mass numbers 8, 9, 12, and 13 are also known. Predict possible modes of radioactive decay for the four radioactive isotopes of boron.
What is the rate of decay from 1.00 mol of radioactive nuclides having the following half-lives: 12,000 years? 12 hours? 12 seconds?
Many transuranium elements, such as plutonium-232, have very short half-lives. (For 232Pu, the half-life is 36 minutes.) However, some, like protactinium-231 (half-life = 3.34 × 104 years), have relatively long half-lives. Use the masses given in the following table to calculate the change
The bromine-82 nucleus has a half-life of 1.0 × 103 min. If you wanted 1.0 g 82Br and the delivery time was 3.0 days, what mass of NaBr should you order (assuming all of the Br in the NaBr was 82Br)?
Assume a constant 14C/12C ratio of 13.6 counts per minute per gram of living matter. A sample of a petrified tree was found to give 1.2 counts per minute per gram. How old is the tree? (For 14C, t1/2 = 5730 years.)
The binding energy for lithium-6 is 3.086 × 1012 J/mol. Calculate the atomic mass of 6Li.
Each of the following isotopes has been used medically for the purpose indicated. Suggest reasons why the particular element might have been chosen for this purpose.a. Cobalt-57, for study of the body’s use of vitamin B12b. Calcium-47, for study of bone metabolismc. Iron-59, for study of red
Photosynthesis in plants can be represented by the following overall equation: Algae grown in water containing some 18O (in H2 18O) evolve oxygen gas with the same isotopic composition as the oxygen in the water. When algae growing in water containing only 16O were furnished carbon dioxide
In the bismuth-214 natural decay series, Bi-214 initially undergoes β decay, the resulting daughter emits an α particle, and the succeeding daughters emit a β and a β particle in that order. Determine the product of each step in the Bi-214 decay series
A proposed system for storing nuclear wastes involves storing the radioactive material in caves or deep mine shafts. One of the most toxic nuclides that must be disposed of is plutonium-239, which is produced in breeder reactors and has a half-life of 24,100 years. A suitable storage place must be
Strontium-90 and radon-222 both pose serious health risks. 90Sr decays by β-particle production and has a relatively long half-life (28.9 years). Radon-222 decays by a-particle production and has a relatively short half-life (3.82 days). Explain why each decay process poses health risks.
Complete the following table with the nuclear particle that is produced in each nuclear reaction. Initial Nuclide 23⁹ Pu 94 214Pb 82 60, 27 99- 43 Tc 93Np Product Nuclide 2351 92 214p 60 Ni 28 44Ru 23⁹Pu 94 Particle Produced
A certain radioactive nuclide has a half-life of 3.00 hours.a. Calculate the rate constant in s-1 for this nuclide.b. Calculate the decay rate in decays/s for 1.000 mole of this nuclide.
Which of the following statement(s) is(are) true?a. A radioactive nuclide that decays from 2.00 × 1021 atoms to 5.0 × 1020 atoms in 16 minutes has a half-life of 8.0 minutes.b. Nuclides with large Z values are observed to be α-particle producers.c. As Z increases, nuclides need a greater
A 0.10-cm3 sample of a solution containing a radioactive nuclide (5.0 × 103 counts per minute per milliliter) is injected into a rat. Several minutes later 1.0 cm3 of blood is removed. The blood shows 48 counts per minute of radioactivity. Calculate the volume of blood in the rat. What assumptions
A reported synthesis of the transuranium element bohrium (Bh) involved the bombardment of berkelium-249 with neon22 to produce bohrium-267. Write a nuclear reaction for this synthesis. The half-life of bohrium-267 is 15.0 seconds. If 199 atoms of bohrium-267 could be synthesized, how much time
Explain the following relationships: ΔG and w, cell potential and w, cell potential and ΔG, cell potential and Q. Using these relationships, explain how you could make a cell in which both electrodes are the same metal and both solutions contain the same compound, but at different concentrations.
Explain why cell potentials are not multiplied by the coefficients in the balanced redox equation. (Use the relationship between ΔG and cell potential to do this.)
If the cell potential is proportional to work and the standard reduction potential for the hydrogen ion is zero, does this mean that the reduction of the hydrogen ion requires no work?
Is the following statement true or false? Concentration cells work because standard reduction potentials are dependent on concentration. Explain.
Assign oxidation numbers to all the atoms in each of the following: a. HNO3b. CuCl2c. O2d. H2O2e. C6H12O6f. Agg. PbSO4h. PbO2i. Na2C2O4j. CO2k. (NH4)2Ce(SO4)3l. Cr2O3
Consider the electrolysis of a molten salt of some metal. What information must you know to calculate the mass of metal plated out in the electrolytic cell?
Look up the reduction potential for Fe3+ to Fe2+. Look up the reduction potential for Fe2+ to Fe. Finally, look up the reduction potential for Fe3+ to Fe. You should notice that adding the reduction potentials for the first two does not give the potential for the third. Why not? Show how you can
The general rule for salt bridges is that anions flow to the anode and cations flow to the cathode. Explain why this is true.
What is wrong with the following statement: The best concentration cell will consist of the substance having the most positive standard reduction potential. What drives a concentration cell to produce a large voltage?
When jump-starting a car with a dead battery, the ground jumper should be attached to a remote part of the engine block. Why?
Which of the following statements concerning corrosion is(are) true? For the false statements, correct them. a. Corrosion is an example of an electrolytic process.b. Corrosion of steel involves the reduction of iron coupled with the oxidation of oxygen.c. Steel rusts more easily in the
Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are 1.0 M and that all partial
Calculate ΔGο and K at 25οC for the reactions in Exercises 37 and 41. Data in Exercise 37 Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, and identify the cathode and anode. Give the overall balanced equation. Assume that all
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are
An electrochemical cell consists of a nickel metal electrode immersed in a solution with [Ni2+] = 1.0 M separated by a porous disk from an aluminum metal electrode.a. What is the potential of this cell at 25οC if the aluminum electrode is placed in a solution in which [Al3+] = 7.2 × 10-3
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 M NH3 that is also 0.010 M in Cu(NH3)42+, what is the cell potential at 25οC?
Cadmium sulfide is used in some semiconductor applications. Calculate the value of the solubility product constant (Ksp) for CdS given the following standard reduction potentials: CdS (s) + 2e →→ Cd(s) + S² (aq) Cd²+ (aq) + 2e → Cd(s) ४० = -1.21 V co = -0.402 V
The electrolysis of BiO+ produces pure bismuth. How long would it take to produce 10.0 g Bi by the electrolysis of a BiO+ solution using a current of 25.0 A?
Aluminum is produced commercially by the electrolysis of Al2O3 in the presence of a molten salt. If a plant has a continuous capacity of 1.00 million A, what mass of aluminum can be produced in 2.00 h?
A factory wants to produce 1.00 × 103 kg barium from the electrolysis of molten barium chloride. What current must be applied for 4.00 h to accomplish this?
It took 2.30 min using a current of 2.00 A to plate out all the silver from 0.250 L of a solution containing Ag+. What was the original concentration of Ag+ in the solution?
A solution containing Pt4+ is electrolyzed with a current of 4.00 A. How long will it take to plate out 99% of the platinum in 0.50 L of a 0.010-M solution of Pt4+?
A solution at 25οC contains 1.0 M Cd2+, 1.0 M Ag+, 1.0 M Au3+, and 1.0 M Ni2+ in the cathode compartment of an electrolytic cell. Predict the order in which the metals will plate out as the voltage is gradually increased.
A solution at 25°C contains 1.0 M Cu2+ and 1.0 × 10–4 M Ag+. Which metal will plate out first as the voltage is gradually increased when this solution is electrolyzed?
Copper can be plated onto a spoon by placing the spoon in an acidic solution of CuSO4(aq) and connecting it to a copper strip via a power source as illustrated below:a. Label the anode and cathode, and describe the direction of the electron flow.b. Write out the chemical equations for the reactions
When aluminum foil is placed in hydrochloric acid, nothing happens for the first 30 seconds or so. This is followed by vigorous bubbling and the eventual disappearance of the foil. Explain these observations.
Calculate the value of the equilibrium constant for the reaction of lead metal in a solution of silver nitrate at 25°C.
Electrolysis has many important industrial applications. What are some of these applications? The electrolysis of molten NaCl is the major process by which sodium metal is produced. However, the electrolysis of aqueous NaCl does not produce sodium metal under normal circumstances. Why? What is
You are told that metal A is a better reducing agent than metal B. What, if anything, can be said about A+ and B+? Explain.
Human DNA contains almost twice as much information as is needed to code for all the substances produced in the body. Likewise, the digital data sent from Voyager II contained one redundant bit out of every two bits of information. The Hubble space telescope transmits three redundant bits for
ΔSsurr is sometimes called the energy disorder term. Explain.
List three different ways to calculate the standard free energy change, ΔGο, for a reaction at 25οC. How is ΔGο estimated at temperatures other than 25οC? What assumptions are made?
Consider the following relationships: Which of these relationships is(are) always true for a reaction at equilibrium? AG° = 1, AH = TAS, Q = 1, AG = AGº, K = 1
The ultimate electron acceptor in the respiration process is molecular oxygen. Electron transfer through the respiratory chain takes place through a complex series of oxidation– reduction reactions. Some of the electron transport steps use iron-containing proteins called cytochromes. All
Hydrogen peroxide can function either as an oxidizing agent or as a reducing agent. At standard conditions, is H2O2 a better oxidizing agent or reducing agent? Explain.
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
Sketch a cell that forms iron metal from iron(II) while changing chromium metal to chromium(III). Calculate the voltage, show the electron flow, label the anode and cathode, and balance the overall cell equation.
Calculate ΔHo , ΔSo , and ΔGo at 25°C for each of the following reactions that occur in the atmosphere. a. C₂H4(g) + O2(g) → CH3CHO(g) + O₂(g) b. 03(g) + NO(g) → NO₂(g) + O₂(g) c. SO3(g) + H₂O(l) → H₂SO4(aq)
Given the following data: calculate ΔGο for the reaction 2C¢Hl) + 15O,(g) C(s) + O(g) H»(g) + }O»(g) 12CO,(g) + 6H2O(l) → CO2(g) H2Ol) AG° = -6399 kJ = AG° = -394 kJ AG° = -237 kJ
For the sublimation of iodine at 25°Cthe values of ΔHo and ΔGo are, respectively, 62 kJ and 19 kJ. Estimate the temperature at which iodine sublimes. Assume ΔHo and ΔSo do not depend on temperature. 1₂(s) → 1₂(g)
Consider the following reaction at 25.0οC:The values of ΔHο and ΔSο are -58.03 kJ/mol and -176.6 J/K ? mol, respectively. Calculate the value of K at 25.0οC. Assuming ΔHο and ΔSο are temperature independent, estimate the value of K at 100.0οC. 2NO₂(g) N₂O4(g)
A reaction has K = 1.9 × 10–14 at 25°C and K = 9.1 × 103 at 227°C. Predict the signs for ΔGo , ΔHo , and ΔSo for this reaction at 25°C. Assume ΔHo and ΔSo do not depend on temperature.
Given the thermodynamic data below, calculate ΔSο and ΔSsurr for the following reaction at 25οC and 1 atm: XeF (g) XeF4(s) + F₂(8)
For rubidium ΔHοvap = 69.0 kJ/mol at 686οC, its boiling point. Calculate ΔSο, q, w, and ΔE for the vaporization of 1.00 mole of rubidium at 686οC and 1.00 atm pressure.
The following reaction occurs in pure water: which is often abbreviated as For this reaction, ΔGο = 79.9 kJ/mol at 25οC. Calculate the value of ΔG for this reaction at 25οC when [OH-] = 0.15 M and [H+] = 0.71 M. (bv)_HO + (bv)+O³H—(1)0¹H + (1)0¹H
Some water is placed in a coffee-cup calorimeter. When 1.0 g of an ionic solid is added, the temperature of the solution increases from 21.5οC to 24.2οC as the solid dissolves. For the dissolving process, what are the signs for ΔSsys, ΔSsurr, and ΔSuniv?
Which of the following statements is(are) true? Explain.a. Oxidation and reduction cannot occur independently of each other.b. Oxidation and reduction accompany all chemical reactions.c. A substance that reacts with oxygen gas will always be oxidized.
Galvanic cells harness spontaneous oxidation–reduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment?

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