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chemical engineering

General Chemistry 9th edition Darrell Ebbing, Steven D. Gammon - Solutions

The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction was 2H2O(l) + 2e → H2(g) + 2OH(aq) Hydroxide ion reacts with lactic acid as soon as it is
A standard electrochemical cell is made by dipping a silver electrode into a 1.0 M Ag solution and a cadmium electrode into a 1.0 M Cd2+ solution. a. What is the spontaneous chemical reaction, and what is the maximum potential produced by this cell? b. What would be the effect on the potential of
A standard electrochemical cell is made by dipping an iron electrode into a 1.0 M Fe2+ solution and a copper electrode into a 1.0 M Cu2+ solution. a. What is the spontaneous chemical reaction, and what is the maximum potential produced by this cell? b. What would be the effect on the potential of
A solution of copper(II) sulfate is electrolyzed by passing a current through the solution using inert electrodes. Consequently, there is a decrease in the Cu2+ concentration and an increase in the hydronium ion concentration. Also, one electrode increases in mass and a gas evolves at the other
Explain the electrochemistry of rusting.
A potassium chloride solution is electrolyzed by passing a current through the solution using inert electrodes. A gas evolves at each electrode, and there is a large increase in pH of the solution. Write the half-reactions that occur at the anode and at the cathode.
A constant current of 1.50 amp is passed through an electrolytic cell containing a 0.10 M solution of AgNO3 and a silver anode and a platinum cathode until 2.48 g of silver is deposited. a. How long does the current flow to obtain this deposit? b. What mass of chromium would be deposited in a
A constant current of 1.25 amp is passed through an electrolytic cell containing a 0.050 M solution of CuSO4 and a copper anode and a platinum cathode until 2.20 g of copper is deposited. a. How long does the current flow to obtain this deposit? b. What mass of silver would be deposited in a
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.50 hours. The electroplating is carried out with an efficiency of 90.0%, resulting in a deposit of 21.221 g of gold. a. How many faradays are required to deposit the gold? b. What is the charge on the
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a. How many faradays are required to deposit the vanadium? b. What is the charge
An electrochemical cell is made by placing a zinc electrode in 1.00 L of 0.200 M ZnSO4 solution and a copper electrode in 1.00 L of 0.0100 M CuCl2 solution. a. What is the initial voltage of this cell when it is properly constructed? b. Calculate the final concentration of Cu2+ in this cell if it
An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.15 M FeSO4 solution and a copper electrode in 1.00 L of 0.036 M CuSO4 solution. a. What is the initial voltage of this cell when it is properly constructed? b. Calculate the final concentration of Cu2+ in this cell if it is
a) Calculate ∆Go for the following cell reaction: Cd(s) Cd2+(aq)|\Co2+(aq)|Co(s) The ∆Gof for Cd2+(aq) is 77.6 kJ/mol. (b) From ∆Go, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Co2+(aq) + 2e → Co(s).
(a) Calculate ∆Go for the following cell reaction: Tl(s)|Tl+(aq)||Pb2+(aq)|Pb(s) The ∆Gof for Tl+(aq) is 32.4 kJ/mol. (b) From ∆Go, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl+(aq) + e → Tl(s)
A voltaic cell is constructed from a half-cell in which a chromium rod dips into a solution of chromium(III) nitrate, Cr(NO3)3, and another half-cell in which a lead rod dips into a solution of lead(II) nitrate, Pb(NO3)2. The two half-cells are connected by a salt bridge. Chromium metal is oxidized
Iron may be protected by coating with tin (tin cans) or with zinc (galvanized iron). Galvanized iron does not corrode as long as zinc is present. By contrast, when a tin can is scratched, the exposed iron underneath corrodes rapidly. Explain the difference between zinc and tin as protective
What are the overall cell reaction and the cell potential for this voltaic cell? Mg(s) WMg2+(aq)||Fe3+(aq) |Fe(s)
The cell potential of a particular voltaic cell with the cell reaction 2Cr(s) + 3Cu2+(aq) → 2Cr3+(aq) + 3 Cu(s) is 1.14 V. What is the maximum electrical work, per mole, that can be obtained from 6.61 g of chromium metal?
Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).
What is the cell potential (Ecell) of a spontaneous cell that is run at 25oC and contains [Cr3+] = 0.10 M and [Ag+] = 1.0 × 104 M?
A strip of aluminum metal is placed into a beaker containing 1.0 M CuSO4. (a) Will a spontaneous reaction occur? (b) If a spontaneous reaction does occur, write the half-reactions and describe what you would observe.
How many grams of hydrogen can be produced by the electrolysis of water with a current of 0.325 A running for 5.00 min?
The following two half-reactions are involved in a voltaic cell. At standard conditions, what species is produced at each electrode? Ag+ + e →Ag Eo = 0.80 V Ni2+ + 2e → Ni Eo = 0.25 V
Consider the following reaction run at standard conditions: Al(s) + Fe2+(aq) → Fe(s) +Al3+(aq) a. Calculate the standard cell potential for this cell from standard free energies of formation (see Appendix C). b. Calculate the equilibrium constant for the reaction. c. How would the value of the
Consider the following cell reaction at 25oC. 2Cr3+(aq) + 3Zn(s) → 3Zn2+(aq) + 2Cr(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain ∆Go for the cell reaction. Use data in Appendix C to calculate ∆Ho; note that Cr(H2O)63+(aq)
Consider the following cell reaction at 25C. 2Cr(s) + 3Fe2+(aq) → 2Cr3 + (aq) + 3Fe(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain ∆Go for the cell reaction. Use data in Appendix C to calculate ∆Ho; note that Cr(H2O)63+(aq)
Under standard conditions for all concentrations, the following reaction is spontaneous at 25oC. O2(g) + 4H + (aq) + 4Br(aq) → 2H2O(l) + 2Br2(l) If [H+] is decreased so that the pH = 3.60, what value will Ecell have, and will the reaction be spontaneous at this [H+]?
Under standard conditions for all concentrations, the following reaction is spontaneous at 25oC. O3(g) + 2H + (aq) + 2Co2+(aq) → O2(g) + H2O(l) + 2Co3+(l) If [H+] is decreased so that the pH = 9.10, what value will Ecell have, and will the reaction be spontaneous at this [H+]?
Under standard conditions for all concentrations, the following reaction is spontaneous at 25oC. O2(g) + 4H+(aq) + 4Br (aq) → 2H2O(l) + 2Br2(l) If [H+] is adjusted by adding a buffer of 0.10 M NaOCN and 0.10 M HOCN (Ka = 3.5 × 10 4), what value will Ecell have, and will the reaction be
Under standard conditions for all concentrations, the following reaction is spontaneous at 25oC. O3(g) + 2H+(aq) + 2Co2+(aq) → O2(g) + H2O(l) + 2Co3+(aq) If [H+] is adjusted by adding a buffer of 0.10 M NaClO and 0.10 M HClO (Ka = 3.5 × 108), what value will Ecell have, and will the reaction be
An electrode is prepared by dipping a silver strip into a solution saturated with silver thiocyanate, AgSCN, and containing 0.10 M SCN. The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.45 V. What is
An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl2, containing 1.00 M Cl. The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is
Potassium was discovered by the British chemist Humphry Davy when he electrolyzed molten potassium hydroxide. What would be the anode reaction?
Briefly explain why different products are obtained from the electrolysis of molten NaCl and the electrolysis of a dilute aqueous solution of NaCl.
Write the Nernst equation for the electrode reaction 2Cl(aq) → Cl2(g) + 2e. With this equation, explain why the electrolysis of concentrated sodium chloride solution might be expected to release chlorine gas rather than oxygen gas at the anode.
You have the following setup to construct a cell under standard conditions. The anode and cathode are iron and silver rods. Using cell notation, the cell isFe(s) |Fe2 + (aq)||Ag + (aq) |Ag(s).a. Complete the figure of the cell by labeling the anode and cathode and showing the corresponding
Consider this cell running under standard conditions: Ni(s) |Ni2 + (aq)||Cu + (aq) | Cu(s) a. Is this cell a voltaic or an electrolytic cell? How do you know? b. Does current flow in this cell spontaneously? c. What is the maximum cell potential for this cell? d. Say the cell is connected to a
Keeping in mind that aqueous Cu2+ is blue and aqueous Zn2+ is colorless, predict what you would observe over a severalday period if you performed the following experiments. a. A strip of Zn is placed into a beaker containing aqueous Zn2+. b. A strip of Cu is placed into a beaker containing aqueous
You place a battery in a flashlight in which all of the electrochemical reactions have reached equilibrium. What do you expect to observe when you turn on the flashlight? Explain your answer.
From an electrochemical standpoint, what metal, other than zinc, would be a reasonable candidate to coat a piece of iron to prevent corrosion (oxidation)?
Pick a combination of two metals from the Standard Reduction Potential table (Table 19.1 or Appendix I) that would result in a cell with a potential of about + 0.90 V. For your answer, write both the half-reactions, write the overall balanced reaction, and calculate the cell potential for your
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a. writing the symbols of the elements and ions in the appropriate areas (both
The zinc–copper voltaic cell shown with this problem is currently running under standard conditions. How would the intensity of light from the bulb change if you were to
The development of lightweight batteries is an ongoing research effort combining many of the physical sciences. You are a member of an engineering team trying to develop a lightweight battery that will effectively react with O2(g) from the atmosphere as an oxidizing agent. A reducing agent must be
Balance the following oxidation-reduction equations. The reactions occur in acidic solution. a. Cr2O72 + C2O4 2 → Cr3+ + CO2 b. Cu + NO3 → Cu2+ + NO c. MnO2 + HNO2 → Mn2+ + NO3 d. PbO2 + Mn2+ + SO4 2 → PbSO4 + MnO4 e. HNO2 + Cr2O7 2 → Cr3+ + NO3
Balance the following oxidation–reduction equations.
Balance the following oxidation–reduction equations. Discuss.
Balance the following oxidation–reduction equations. Discuss in detail.
Balance the following oxidation-reduction equations. The reactions occur in acidic or basic aqueous solution, as indicated. a. H2S + NO3 → NO2 + S8 (acidic) b. NO3 + Cu → NO + Cu2+ (acidic) c. MnO4 + SO2 → SO42 + Mn2+ (acidic) d. Bi(OH)3 + Sn(OH)3 → Sn(OH)62 + Bi
Balance the following oxidation-reduction equations. The reactions occur in acidic or basic aqueous solution, as indicated. a. Hg22+ + H2S → Hg + S8 (acidic) b. S2 + I2 → SO42 + I (basic) c. Al + NO3 →Al(OH)4 + NH3 (basic) d. MnO4 + C2O4 2 → MnO2 + CO2 (basic)
Balance the following oxidation-reduction equations. The reactions occur in acidic or basic aqueous solution, as indicated. a. MnO4 + I → MnO2 + IO3 (basic) b. Cr2O72 + Cl → Cr3+ + Cl2 (acidic) c. S8 + NO3 + SO2 + NO (acidic) d. H2O2 MnO4 → O2 + MnO2 (basic) e. Zn + NO3 → Zn2+ +
Balance the following oxidation-reduction equations. The reactions occur in acidic or basic aqueous solution, as indicated. a. Cr2O72 + H2O2 + Cr3+ + O2 (acidic) b. CN + MnO4 + CNO + MnO2 (basic) c. Cr(OH)4 + OCl + CrO42 + Cl (basic) d. Br2 + SO2 + Br + SO42 (acidic) e. CuS + NO3 + Cu2+
Voltaic cell is constructed from the following halfcells: a magnesium electrode in magnesium sulfate solution and a nickel electrode in nickel sulfate solution. The halfreactions are Mg(s) → Mg2 + (aq) + 2e Ni2 + (aq) + 2e → Ni(s) Sketch the cell, labeling the anode and cathode (and the
Half-cells were made from a nickel rod dipping in a nickel sulfate solution and a copper rod dipping in a copper sulfate solution. The half-reactions in a voltaic cell using these half-cells were Cu2+(aq) + 2e→ Cu(s) Ni(s) → Ni2+ (aq) + 2e Sketch the cell and label the anode and cathode,
Zinc reacts spontaneously with silver ion. Zn(s) + 2Ag + (aq) → Zn2 + (aq) + 2Ag(s) Describe a voltaic cell using this reaction. What are the halfreactions?
Iron reacts spontaneously with copper(II) ion. Fe(s) + Cu2 + (aq) → Fe2 + (aq) + Cu(s) Obtain half-reactions for this, and then describe a voltaic cell using these half-reactions
A silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V). The button form of this cell is used in watches, hearing aids, and other electronic devices. The half-reactions are Zn(s) + 2OH(aq) → Zn(OH)2(s) + 2e Ag2O(s) + H2O(l) + 2e → 2Ag(s) + 2OH(aq) Identify
A mercury battery, used for hearing aids and electric watches, delivers a constant voltage (1.35 V) for long periods. The half-reactions are HgO(s) + H2O(l) + 2e → Hg(l) + 2OH (aq) Zn(s) + 2OH (aq) → Zn(OH)2(s) + 2e Which half-reaction occurs at the anode and which occurs at the cathode? What
Write the cell notation for a voltaic cell with the following half-reactions. Ni(s)→ Ni2 + (aq) + 2e Pb2 + (aq) + 2e → Pb(s)
Why is it necessary to measure the voltage of a voltaic cell when no current is flowing to obtain the cell potential?
Write the cell notation for a voltaic cell with the following half-reactions. Al(s) → Al3+ (aq) + 3e 2H + (aq) + 2e → H2(g)
Give the notation for a voltaic cell constructed from a hydrogen electrode (cathode) in 1.0 M HCl and a nickel electrode (anode) in 1.0 M NiSO4 solution. The electrodes are connected by a salt bridge.
A voltaic cell has an iron rod in 0.30 M iron(III) chloride solution for the cathode and a zinc rod in 0.20 M zinc sulfate solution for the anode. The half-cells are connected by a salt bridge. Write the notation for this cell.
Write the overall cell reaction for the following voltaic cell. Fe(s) |Fe2+(aq)||Ag + (aq)|Ag(s)
Write the overall cell reaction for the following voltaic cell. Pt|H2(g) |H+(aq)||Br2(l) | Br(aq)|Pt
Consider the voltaic cell Cd(s) |Cd2+(aq) || Ni2+(aq) | Ni(s) Write the half-cell reactions and the overall cell reaction. Make a sketch of this cell and label it. Include labels showing the anode, cathode, and direction of electron flow.
Consider the voltaic cell Zn(s) | Zn2+(aq)||Cr3+(aq) |Cr(s) Write the half-cell reactions and the overall cell reaction. Make a sketch of this cell and label it. Include labels showing the anode, cathode, and direction of electron flow.
A voltaic cell whose cell reaction is 2Fe3+(aq) + Zn(s) → 2Fe2+(aq) + Zn2+(aq) has a cell potential of 0.72 V. What is the maximum electrical work that can be obtained from this cell per mole of iron(III) ion?
A particular voltaic cell operates on the reaction Zn(s) + Cl2(g) → Zn2+(aq) + 2Cl(aq) giving a cell potential of 0.853 V. Calculate the maximum electrical work generated when 20.0 g of zinc metal is consumed.
What is the maximum work you can obtain from 30.0 g of nickel in the following cell when the cell potential is 0.97 V? Ni(s)|Ni2+(aq)||Ag + (aq) | Ag(s)
How are standard electrode potentials defined?
Calculate the maximum work available from 50.0 g of aluminum in the following cell when the cell potential is 1.15 V. Al(s) |Al3+ (aq)||H + (aq) |O2(g) |Pt That O2 is reduced to H2O.
Order the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4 (aq); NO3 (aq) (in acidic solution).
Order the following oxidizing agents by increasing strength under standard-state conditions: Ag + (aq); I2(aq); MnO4 (aq) (in acidic solution).
Consider the reducing agents Cu + (aq), Zn(s), and Fe(s). Which is strongest? Which is weakest?
Consider the reducing agents Sn2+(aq), Cu(s), and I(aq). Which is strongest? Which is weakest?
Consider the following reactions. Are they spontaneous in the direction written, under standard conditions at 25oC? a. Sn4+(aq) + 2Fe2+(aq) → Sn2+(aq) + 2Fe3 + (aq) b. 4MnO4 (aq) + 12H+(aq) → 4Mn2+(aq) + 5O2(g) + 6H2O(l)
Answer the following questions by referring to standard electrode potentials at 25oC.
What would you expect to happen when chlorine gas, Cl2, at 1 atm pressure is bubbled into a solution containing 1.0 M F and 1.0 M Br at 25oC? Write a balanced equation for the reaction that occurs.
Dichromate ion, Cr2O72, is added to an acidic solution containing Br and Mn2+. Write a balanced equation for any reaction that occurs. Assume standard conditions at 25oC.
Calculate the standard cell potential of the following cell at 25oC. Cr(s) |Cr3+(aq)||Hg2 2+(aq) |Hg(l)
Calculate the standard cell potential of the following cell at 25oC. Sn(s) |Sn2+(aq)|Cu2+(aq) | Cu(s)
What is the standard cell potential you would obtain from a cell at 25oC using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3 + (aq)?
What is the standard cell potential you would obtain from a cell at 25oC using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?
Calculate the standard free-energy change at 25C for the following reaction. 3Cu(s) + 2NO3 (aq) + 8H+(aq)→ 3Cu2+(aq) + 2NO(g) + 4H2O(l)
Calculate the standard free-energy change at 25C for the following reaction. 4Al(s) + 3O2(g) + 12H + (aq) → 4Al3 + (aq) + 6H2O(l) Use standard electrode potentials.
What is ∆Go for the following reaction? 2I(aq) + Cl2(g) → I2(s) + 2Cl(aq) Use data given in Table 19.1.
Using electrode potentials, calculate the standard freeenergy change for the reaction
Calculate the standard cell potential at 25oC for the following cell reaction from standard free energies of formation (Appendix C). Mg(s) + 2Ag+ (aq) → Mg2+(aq) + 2Ag(s
Calculate the standard cell potential at 25oC for the following cell reaction from standard free energies of formation (Appendix C). 2Al(s) + 3Cu2+(aq) → 2Al3+(aq) + 3Cu(s)
Calculate the standard cell potential of the lead storage cell whose overall reaction is PbO2(s) + 2HSO4 (aq) + 2H+(aq) + Pb(s) → 2PbSO4(s) + 2H2O(l)
Give the mathematical relationships between the members of each possible pair of the three quantities ∆Go, ∆Eo cell, and K.
Calculate the standard cell potential of the cell corresponding to the oxidation of oxalic acid, H2C2O4, by permanganate ion, MnO4 . 5H2C2O4(aq) + 2MnO4 (aq) + 6H + (aq) → 10CO2(g) + 2Mn2 + (aq) + 8H2O(l) See Appendix C for free energies of formation; ∆Gof for H2C2O4(aq) is 698 kJ.
Calculate the equilibrium constant K for the following reaction at 25C from standard electrode potentials. Fe3 + (aq) + Cu(s)→ Fe2+(aq) + Cu2+(aq) The equation is not balanced.
Calculate the equilibrium constant K for the following reaction at 25C from standard electrode potentials. Sn4+(aq) + 2Hg(l → Sn2+(aq) + Hg2 2+(aq) The equation is not balanced.
Copper(I) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with itself. 2Cu + (aq) → Cu(s) + Cu2+(aq) Calculate the equilibrium constant at 25oC for this reaction, using appropriate values of electrode potentials.
Use electrode potentials to calculate the equilibrium constant at 25oC for the reactionSee Appendix I for data.
Calculate the cell potential of the following cell at 25oC. Cr(s) | Cr3+(1.0 × 103 M)||Ni2+(1.5 M) |Ni(s)
What is the cell potential of the following cell at 25oC? Ni(s) |Ni2+(1.0 M)||Sn2+(1.0 × 104 M)|Sn(s)
Calculate the cell potential of a cell operating with the following reaction at 25oC, in which [MnO4 ] = 0.010 M, [Br] = 0.010 M, [Mn2+] = 0.15 M, and [H+] = 1.0 M. 2MnO4(aq) + 10Br(aq) + 16H+ (aq) → 2Mn2+(aq) + 5Br2(l) + H2O(l)

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