Problem 1
In the Brønsted–Lowry concept of acids and bases, acid– base reactions are viewed as proton-transfer reactions. The stronger the acid, the weaker is its conjugate base. If we were to think of redox reactions in a similar way, what particle would be analogous to the proton? Would strong oxidizing agents be analogous to strong acids or strong bases? [Sections 20.1 and 20.2]
Problem 3a
The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.
(a) Does the process represent oxidation or reduction?
Problem 3b
The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.
(b) Is the electrode the anode or cathode?
Problem 3c
The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.
(c) Why are the atoms in the electrode represented by larger spheres than those in the solution? [Section 20.3]
Problem 4
Assume that you want to construct a voltaic cell that uses the following half-reactions: A2+1aq2 + 2 e- ¡ A1s2 Ered ° = -0.10 V B2+1aq2 + 2 e- ¡ B1s2 E°red = -1.10 V You begin with the incomplete cell pictured here in which the electrodes are immersed in water.
(a) What additions must you make to the cell for it to generate a standard emf?
Problem 6
Consider the following table of standard electrode potentials for a series of hypothetical reactions in an aqueous solution: reduction half-reaction E °(V) (c) Which substance(s) can oxidize C2+?
Problem 8c
Consider the following voltaic cell:
(c) What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10?
Problem 10b
The electrodes in a silver oxide battery are silver oxide 1Ag2O2 and zinc (b) Which battery do you think has an energy density most similar to the silver oxide battery: a Li-ion battery, a nickel– cadmium battery, or a lead–acid battery? [Section 20.7]
Problem 11
Bars of iron are put into each of the three beakers as shown here. In which beaker—A, B, or C—would you expect the iron to show the most corrosion ? [Section 20.8]
Problem 12a
Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (a) What is the most common oxidation number for Mg when it is part of a salt?
Problem 12b
Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (b) Chlorine gas is evolved as voltage is applied in the cell. Knowing this, identify the electrolyte.
Problem 12c
Magnesium, the element, is produced commercially by electrolysis from a molten salt (the 'electrolyte') using a cell similar to the one shown here. (c) Recall that in an electrolytic cell the anode is given the + sign and the cathode is given the – sign, which is the opposite of what we see in batteries. What half-reaction occurs at the anode in this electrolytic cell?
Problem 13b
(b) On which side of an oxidation half-reaction do the electrons appear?
Problem 15a
Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons.
Problem 15c
Indicate whether each of the following statements is true or false: (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.
Problem 16c
Indicate whether each of the following statements is true or false: (c) An oxidizing agent is needed to convert CO into CO2.
Problem 17b
For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (b) 2 Hg2+(aq) + N2H4(aq) → 2 Hg(l) + N2(g) + 4 H+(aq)
Problem 18a
For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) 2 MnO4-(aq) + 3 S2-(aq + 4 H2O(l) → 3 S(s) + 2 MnO2(s) + 8 OH-(aq)
Problem 19a
Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) PBr3(l) + 3 H2O(l) → H3PO3(aq) + 3 HBr(aq)
Problem 19b
Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (b) NaI(aq) + 3 HOCl(aq) → NaIO3(aq) + 3 HCl(aq)
Problem 20a
Indicate whether the following balanced equations involve oxidation–reduction. If they do, identify the elements that undergo changes in oxidation number. (a) 2 AgNO3(aq) + CoCl2(aq) → 2 AgCl(s) + Co(NO3)2(aq)
Problem 21a
At 900 °C, titanium tetrachloride vapor reacts with molten magnesium metal to form solid titanium metal and molten magnesium chloride. (a) Write a balanced equation for this reaction.
Problem 22c
Hydrazine 1N2H42 and dinitrogen tetroxide 1N2O42 form a self-igniting mixture that has been used as a rocket propellant. The reaction products are N2 and H2O. (c) Which substance serves as the reducing agent and which as the oxidizing agent?
Problem 23b
Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (b) TiO21s2 ¡ Ti2+1aq2 (acidic solution)
Problem 24
Complete and balance the following half-reactions in basic solution. In each case, indicate whether the half-reaction is an oxidation or a reduction.
a. OH−(𝑎𝑞)⟶O2(𝑔)
b. SO32−(𝑎𝑞)⟶SO42−(𝑎𝑞)
c. N2(𝑔)⟶NH3(𝑔)
d. HO2−(𝑎𝑞)⟶OH−(𝑎𝑞)
Problem 24b
Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (f) SO32-1aq2 ¡ SO42-1aq2 (basic solution)
Problem 25
Complete and balance the following half-reactions in basic solution. In each case, indicate whether the half-reaction is an oxidation or a reduction.
a. O2(𝑔)⟶H2O(𝑙)
b. Mn2+(𝑎𝑞)⟶MnO2(𝑠)
c. Cr(OH)3(𝑠)⟶CrO42−(𝑎𝑞)
d. N2H4(𝑎𝑞)⟶N2(𝑔)
Problem 25c
Complete and balance the following half-reactions in basic solution. In each case, indicate whether the half-reaction is an oxidation or a reduction. c. Cr(OH)3(𝑠)⟶CrO42−(𝑎𝑞)
Problem 26b
Complete and balance the following half-reactions in acidic solution. In each case indicate whether the half-reaction is an oxidation or a reduction. b. H2SO3(𝑎𝑞)⟶SO42−(𝑎𝑞)
Problem 27a
Complete and balance the following equations, and identify the oxidizing and reducing agents: (a) Cr2O72-1aq2 + I-1aq2 ¡ Cr3+1aq2 + IO3-1aq2 (acidic solution)
Ch.20 - Electrochemistry
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