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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

The enzyme lipase catalyzes the hydrolysis of esters of fatty acids. The hydrolysis of p-nitrophenyloctanoate was followed by measuring the appearance of p-nitrophenol in the reaction mixture:The
The structure of methyl methacrylate is given in Table 23.12. Draw the structure of a polymethyl methacrylate (PMMA) polymer that has four monomer units. (PMMA has excellent optical properties and is
Three different compounds with the formula C2H2Cl2 are known.(a) Two of these compounds are geometric isomers. Draw their structures.(b) The third compound is a structural isomer of the other two.
Draw the structure of 2-butanol. Identify the chiral carbon atom in this compound. Draw the mirror image of the structure you first drew. Are the two molecules superimposable?
Draw the structure and name the product formed if the following alcohols are oxidized. Assume an excess of the oxidizing agent is used. If the alcohol is not expected to react with a chemical
Voodoo lilies depend on carrion beetles for pollination. Carrion beetles are attracted to dead animals, and because dead and putrefying animals give off the horrible-smelling amine cadaverine, the
Consider the reactions of C3H7OH.(a) Name the reactant C3H7OH.(b) Draw a structural isomer of the reactant, and give its name.(c) Name the product of reaction A.(d) Name the product of reaction B.
(a) According to the genetic code in Table 24.1, which amino acid is selected by the mRNA codon GAA?(b) What is the sequence in the original DNA that led to this codon being present in the mRNA?(c)
There is a high barrier to rotation around a carbon–carbon double bond, whereas the barrier to rotation around a carbon–carbon single bond is considerably smaller. Use the orbital overlap model
If Ka for a weak acid is 2.4 × 10−11, what is the value of pKa?
Kp for the following reaction is 0.16 at 25°C:The enthalpy change for the reaction at standard conditions is +16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the
The chapter opening photograph (page 670) showed how the cobalt(II) chloride equilibrium responded to temperature changes.(a) Look back at that photograph. Is the conversion of the red cation to the
Explain why benzenesulfonic acid is a Brønsted acid. H-0: :0-S :0: benzenesulfonic acid
m-Nitrophenol, a weak acid, can be used as a pH indicator because it is yellow at a pH above 8.6 and colorless at a pH below 6.8. If the pH of a 0.010 M solution of the compound is 3.44, calculate
Mercury vapor is dangerous because breathing it brings this toxic element into the lungs. We wish to estimate the vapor pressure of mercury at two different temperatures from the following
Chloroacetic acid, ClCH2CO2H, is a moderately weak acid (Ka = 1.40 × 10−3). If you dissolve 94.5 mg of the acid in water to give 125 mL of solution, what is the pH of the solution?
For each of the following electrochemical cells, write equations for the oxidation and reduction half-reactions and for the overall reaction. (a) Cu(s) | Cu²+ (aq) || Fe³+ (aq), Fe²+ (aq) |
In Chapter 13, you learned that entropy, as well as enthalpy, plays a role in the solution process. If ΔH° for the solution process is zero, explain how the process can be driven by entropy.
Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.25 A of current for 1.00 hour. What is the minimum mass of the cadmium that must be used to make the anode in this cell?
Use E° values to predict which of the following metals, if coated on iron, will provide cathodic protection against corrosion to iron.(a) Cu(b) Mg(c) Ni(d) Sn
In the presence of oxygen and water, two half-reactions responsible for the corrosion of iron areCalculate the the standard potential, E°, and decide whether the reaction is product-favored at
Use E° values to predict which of the following metals, if coated on nickel, will provide cathodic protection against corrosion to nickel.(a) Cu(b) Mg(c) Zn(d) Cr
In the presence of oxgyen and acid, two half-reactions responsible for the corrosion of iron areCalculate the the standard potential, E°, and decide whether the reaction is product-favored at
Balance the following equations. (a) Zn(s) + VO²+ (aq) → Zn²+ (aq) + V³+ (aq) (b) Zn(s) + VO3(aq) → V2+ (aq) + Zn²+ (aq) (c) Zn(s) + CIO- (aq) → Zn(OH)₂(s) + Cl¯(aq) (d) CIO- (aq) +
Write balanced equations for the following half-reactions.(a) UO2+(aq) → U4+(aq) (acid solution)(b) ClO3−(aq) → Cl−(aq) (acid solution)(c) N2H4(aq) → N2(g) (basic solution)(d) ClO−(aq)
Magnesium metal is oxidized, and silver ions are reduced in a voltaic cell using Mg2+(aq, 1 M) | Mg and Ag+(aq, 1 M) | Ag half-cells.(a) Label each part of the cell.(b) Write equations for the
You want to set up a series of voltaic cells with specific cell potentials. A Zn2+(aq, 1.0 M) | Zn(s) half-cell is in one compartment. Identify several half-cells that you could use so that the cell
A cell is constructed using the following half-reactions:(a) What reactions should be observed at the anode and cathode?(b) Calculate the solubility product constant, Ksp, for Ag2SO4. Ag+ (aq) + e
A potential of 0.142 V is recorded (under standard conditions) for a voltaic cell constructed using the following half reactions:(a) What is the standard reduction potential for the anode
Which of the following reactions is (are) product-favored at equilibrium? (a) Zn(s) + 1₂(s) → Zn²+ (aq) + 2 I¯ (aq) (b) 2 Cl (aq) + ₂(s)→ Cl₂(g) + 2 [¯ (aq) (c) 2 Nat (aq) + 2 Cl (aq)
You want to set up a series of voltaic cells with specific cell potentials. The Ag+(aq, 1.0 M) | Ag(s) half-cell is one of the compartments. Identify several half-cells that you could use so that the
In the table of standard reduction potentials, locate the half-reactions for the reductions of the following metal ions to the metal: Sn2+(aq), Au+(aq), Zn2+(aq), Co2+(aq), Ag+(aq), Cu2+(aq). Among
In the table of standard reduction potentials, locate the half-reactions for the reductions of the following nonmetals: F2, Cl2, Br2, I2 (reduction to halide ions), and O2, S, Se (reduction to H2X in
The following half-cells are available:(i) Ag+(aq, 1.0 M) | Ag(s)(ii) Zn2+(aq, 1.0 M) | Zn(s)(iii) Cu2+(aq, 1.0 M) | Cu(s)(iv) Co2+(aq, 1.0 M) | Co(s)Linking any two half-cells makes a voltaic cell.
Four voltaic cells are set up. In each, one half-cell contains a standard hydrogen electrode. The second half-cell is one of the following:(i) Cr3+(aq, 1.0 M) | Cr(s)(ii) Fe2+(aq, 1.0 M) | Fe(s)(iii)
The reaction occurring in the cell in which Al2O3 and aluminum salts are electrolyzed is Al3+(aq) +3 e− → Al(s). If the electrolysis cell operates at 5.0 V and 1.0 × 105 A, what mass of aluminum
Use the standard reduction potentials (Appendix M) for the half-reactions Hg2Cl2(s) + 2e− → 2 Hg(ℓ) + 2 Cl−(aq) and Hg22+(aq) + 2 e− → 2 Hg(ℓ) to calculate the value of Ksp for
Use the standard reduction potentials (Appendix M) for the half-reactions [AuCl4]−(aq) + 3 e− → Au(s) + 4 Cl−(aq) and Au3+(aq) + 3 e− → Au(s) to calculate the value of Kformation for the
In 1937, R. Schwartz and M. Schmiesser prepared a yellow-orange bromine oxide (BrO2) by treating Br2 with ozone in a fluorocarbon solvent. Many years later, J. Pascal found that, on heating, this
What is the value of E° for the following half-reaction? Ag CrO4(s) + 2e 2 Ag(s) + 2 Ag(s) + CrO-(aq)
The standard potential, E°, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, ΔrG°, for the reaction?
An electrolysis cell for aluminum production operates at 5.0 V and a current of 1.0 × 105 A. Calculate the number of kilowatt-hours of energy required to produce 1 metric ton (1.0 × 103 kg) of
Electrolysis of molten NaCl is done in cells operating at 7.0 V and 4.0 × 104A. What mass of Na(s) and Cl2(g) can be produced in 1 day in such a cell? What is the energy consumption in
A current of 0.0100 A is passed through a solution of rhodium sulfate, causing reduction of the metal ion to the metal. After 3.00 hours, 0.038 g of Rh has been deposited. What is the charge on the
A current of 0.44 A is passed through a solution of ruthenium nitrate causing reduction of the metal ion to the metal. After 25.0 minutes, 0.345 g of Ru has been deposited. What is the charge on the
The total charge that can be delivered by a large dry cell battery before its voltage drops too low is usually about 35 amp-hours. (One amp-hour is the charge that passes through a circuit when 1 A
Chlorine gas is obtained commercially by electrolysis of brine (a concentrated aqueous solution of NaCl). If the electrolysis cells operate at 4.6 V and 3.0 × 105 A, what mass of chlorine can be
Write equations for the half-reactions that occur at the anode and cathode in the electrolysis of molten KBr. What are the products formed at the anode and cathode in the electrolysis of aqueous KBr?
The products formed in the electrolysis of aqueous CuSO4 are Cu(s) and O2(g). Write equations for the anode and cathode reactions.
Predict the products formed in the electrolysis of an aqueous solution of CdSO4.
In the electrolysis of HNO3(aq), hydrogen is produced at the cathode. According to a table of reduction potentials, NO3−(aq) is easier to reduce than H+(aq). Suggest a possible reason why H2 formed
The metallurgy of aluminum involves electrolysis of Al2O3 dissolved in molten cryolite (Na3AlF6) at about 950°C. Aluminum metal is produced at the cathode. Predict the anode product and write
A voltaic cell is set up utilizing the reactionUnder standard conditions, the expected potential is 0.45 V. Predict whether the potential for the voltaic cell will be higher, lower, or the same as
Two half-cells, Pt | Fe3+(aq, 0.50 M), Fe2+(aq, 1.0 × 10−5 M) and Hg2+(aq, 0.020 M) | Hg, are constructed and then linked together to form a voltaic cell. Which electrode is the anode? What will
Calculate the cell potential for the following cell:Will this reaction be more or less favorable at lower pH? To determine this, calculate the cell potential for a reaction in which [H+(aq)] is 1.0
A voltaic cell set up utilizing the reactionhas a cell potential of 0.45 V at 298 K. Describe how the potential of this cell will change as the cell is discharged. At what point does the cell
Calculate equilibrium constants for the following reactions at 298 K. Indicate whether the equilibrium as written is reactant- or product-favored at equilibrium. Co²+ (aq) + Ni(s) (a) Co(s) +
Two Ag+(aq) | Ag(s) half-cells are constructed. The first has [Ag+] = 1.0 M, the second has [Ag+] = 1.0 × 10−5 M. When linked together with a salt bridge and external circuit, a cell potential is
Calculate equilibrium constants for the following reactions at 298 K. Indicate whether the equilibrium as written is reactant- or product-favored at equilibrium. (a) 2 Cl(aq) + Br₂(e) (b) Fe²+
Use the table of standard reduction potentials (Appendix M) to calculate ΔrG° for the following reactions at 298 K.Data given in Appendix M (a) CIO3(aq) + 5 Cl(aq) + 6 H+ (aq) → 3 Cl₂(g) + 3
In 2005, global SO2 emission was estimated to be 12.83 Gg (gigagrams). According to the EPA, 71% of SO2 emissions into the atmosphere is from coalfired power plants. How much coal (in metric tons)
Chlorine atoms are formed by photochemical reactions of chlorofluorocarbons in the upper atmosphere. Using the average bond energy of the C—Cl bond in Table 8.8, calculate the wavelength of
The formation of NO from N2 and O2 is unfavorable at 298 K, but it becomes increasingly favored at high temperatures such as those in an automobile cylinder. Using data (ΔfH°, S° and ΔfG°) in
Acetonitrile, CH3CN, is an important solvent. The chemical is normally available as a by-product of the manufacture of acrylonitrile, CH2=CHCN, the building block of polyacrylonitrile, a widely used
The refrigerating liquids in air conditioners and refrigerators are largely chlorofluorocarbons (CFCs) and hydrochlorofluorocarbons (HCFCs). Among the latter family of compounds is the refrigerant
The nitrogen cycle (Figure 20.1) shows the oxidation of NH4+, first to NO2− and then the subsequent oxidation of NO2− to NO3−. Write balanced equations for each of these half-reactions (in acid
Refer to the figure below and Figure 20.25, which show the fraction of species in solution [alpha (α)] as a function of pH. The following questions are in regard to the equilibria involved in an
Here we want to compare ethanol (C2H5OH) and gasoline as fuels. We will use isooctane (C8H18) as a substitute for gasoline. (Isooctane is one of the many hydrocarbons in gasoline, and its enthalpy of
Steps have been taken to limit phosphorus is surface water. However, the amounts of nitrogen containing species in surface water can also be a problem because they also promote excessive growth of
Bromine is obtained from brine wells. The process involves treating water containing bromide ion with Cl2 and extracting the Br2 from the solution using an organic solvent. Write a balanced equation
The mineral claudetite contains the element arsenic in the form of arsenic(III) oxide, As2O3. The As2O3 in a 0.562-g sample of the impure mineral was converted first to H3AsO3 and then titrated with
Imagine the following experiment: You have a large graduated cylinder containing 100. mL of liquid water at 0°C. You drop an ice cube with a volume of 25 cm3 into the cylinder. Ice has a density of
The hypohalite ions, XO−, are the anions of weak acids. Calculate the pH of a 0.10 M solution of NaClO. What is the concentration of HClO in this solution?
To prepare chlorine from chloride ion a strong oxidizing agent is required. The dichromate ion, Cr2O72−, is one example (Figure 21.35). Consult the table of standard reduction potentials (Appendix
If an electrolytic cell for producing F2 (Figure 21.34) operates at 5.00 × 103 A (at 10.0 V), what mass of F2 can be produced per 24-hour day? Assume the conversion of F− to F2 is 100%.Data given
Halogens combine with one another to produce interhalogens such as BrF3. Sketch a possible molecular structure for this molecule, and decide if the F—Br—F bond angles will be less than or greater
In which of the following species is Xe in the + 4 oxidation state?(a) XeOF4(b) Xe2F3+(c) XeF3+(d) XeO64−
Predict the electron pair geometry for the xenon atom in XeOF4.(a) Linear(b) Trigonal bipyramid(c) Trigonal planar(d) Octahedral(e) Tetrahedral
The standard enthalpy of formation of XeF4 is −218 kJ/mol. Use this value and the enthalpy of dissociation of the F—F bond to calculate the Xe—F bond dissociation enthalpy.
Draw the Lewis electron dot structure for XeO3F2. What is its electron-pair geometry and its molecular geometry?
Argon is present in dry air to the extent of 0.93% by volume. What quantity of argon is present in 1.00 L of air? If you wanted to isolate 1.00 mol of argon, what volume of air would you need at 1.00
The reaction of XeF6 with water gives a yellow solution from which solid xenon trioxide, XeO3, can be isolated (using extreme caution).(a) Write a balanced equation for this reaction.(b) What is the
For each of the third-period elements (Na through Ar), identify the following:(a) Whether the element is a metal, nonmetal, or metalloid.(b) The color and appearance of the element.(c) The state of
Consider the chemistries of C, Si, Ge, and Sn.(a) Write a balanced chemical equation to depict the reaction of each element with elemental chlorine.(b) Describe the bonding in each of the products of
Consider the chemistries of the elements potassium, calcium, gallium, germanium, and arsenic.(a) Write a balanced chemical equation depicting the reaction of each element with elemental chlorine.(b)
When BCl3 gas is passed through an electric discharge, small amounts of the reactive molecule B2Cl4 are produced. (The molecule has a B—B covalent bond.)(a) Draw a Lewis electron dot structure for
Complete and balance the following equations.(a) KClO3 + heat →(b) H2S(g) + O2(g) →(c) Na(s) + O2(g) →(d) P4(s) + KOH(aq) + H2O(ℓ) →(e) NH4NO3(s) + heat →(f) In(s) + Br2(ℓ) →(g)
(a) Heating barium oxide in pure oxygen gives barium peroxide. Write a balanced equation for this reaction.(b) Barium peroxide is an excellent oxidizing agent. Write a balanced equation for the
Using data in Appendix L, calculate ΔrG° values for the decomposition of MCO3 to MO and CO2 where M = Mg, Ca, Ba. What is the relative tendency of these carbonates to decompose?Data given in
Worldwide production of silicon carbide, SiC, is several hundred thousand tons annually. If you want to produce 1.0 × 105 metric tons of SiC, what mass (metric tons) of silicon sand (SiO2) will you
To store 2.88 kg of gasoline with an energy equivalence of 1.43 × 108 J requires a volume of 4.1 L. In comparison, 1.0 kg of H2 has the same energy equivalence. What volume is required if this
Metals react with hydrogen halides (such as HCl) to give the metal halide and hydrogen:The free energy change for the reaction is ΔrG° = ΔfG°(MXn) − n ΔfG°[HX(g)].(a) ΔfG° for HCl(g) is
Ammonium perchlorate is used as the oxidizer in solid-fuel rockets. Assume that one launch requires 700. tons (6.35 × 105 kg) of the salt, and the salt decomposes according to the equation on page
Halogens form polyhalide ions. Sketch Lewis electron dot structures and molecular structures for the following ions:(a) I3−(b) BrCl2−(c) ClF2+(d) An iodide ion and two iodine molecules form the
The steering rockets in space vehicles use N2O4 and a derivative of hydrazine, 1,1-dimethylhydrazine (Study Question 5.86). This mixture is called a hypergolic fuel because it ignites when the
The standard enthalpy of formation of OF2 gas is +24.5 kJ/mol. Calculate the average O—F bond enthalpy.
Calcium fluoride can be used in the fluoridation of municipal water supplies. If you want to achieve a fluoride ion concentration of 2.0 × 10−5 M, what mass of CaF2 must you use for 1.0 × 106 L
Liquid HCN is dangerously unstable with respect to trimer formation—that is, formation of (HCN)3 with a cyclic structure.(a) Propose a structure for this cyclic trimer.(b) Estimate the energy of
Use ΔfH° data in Appendix L to calculate the enthalpy change of the reactionSpeculate on whether such a reaction could be used to “fix” nitrogen. Would research to find ways to accomplish this
Phosphorus forms an extensive series of oxoanions.(a) Draw a structure, and give the charge for an oxophosphate anion with the formula [P4O13]n−. How many ionizable H atoms should the completely

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