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(a) What is the reduction potential of the half reaction in which V2+ is reduced to V?
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(b) Give the balanced half equation and accompanying E° value for the reduction half-reaction with the largest (most positive) E° value that involves a pair of species indicated in the Frost diagram.
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(c) Indicate which species, if any, will undergo disproportionation.
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(d) Give the balanced reduction half-equation and accompanying E° value for the reduction of VO2+ to V2+.
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(e) In the Pourbaix diagram for vanadium a diagonal line separates the species VO2+ and V3+. Give the equation of this line, which relates pH and E.
![time 121 +2 +2 = 8 minutes] Question 8 0) is shown below The Frost diagram for vanadium under acidic conditions (pH Oxidation](//img.homeworklib.com/images/814bde24-9839-496e-ad4e-12ee4d7e3309.png?x-oss-process=image/resize,w_560)
![time 121 +2 +2 = 8 minutes] Question 8 0) is shown below The Frost diagram for vanadium under acidic conditions (pH Oxidation](http://img.homeworklib.com/images/814bde24-9839-496e-ad4e-12ee4d7e3309.png?x-oss-process=image/resize,w_560)
Homework Answers
a) 
c) any species of vanadium will not under go the
disproportionation process.
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(a) What is the reduction potential of the half reaction in
which V2+ is reduced to...
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction....
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Cr3+(aq) + 3e — Cr(s) Al(s)—+A13+(aq) + 3e (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. <> Submit Answer Retry Entire Group 9 more group attempts remaining When the following half reaction is balanced under acidic conditions, what are the coefficients of the species shown? NO3 + H —— NO + H2O In the above...
Question 1: Consider the following oxidation-reduction reaction: I−(aq)+Cu+(aq)→IO4−(aq)+Cu(s) A: What are the initial a...
Question 1: Consider the following oxidation-reduction reaction: I−(aq)+Cu+(aq)→IO4−(aq)+Cu(s) A: What are the initial and final oxidation states of iodine? B: What are the initial and final oxidation states of copper? C: What element is reduced? D:What is the reducing agent? E: What element is oxidized? F: What is the oxidizing agent? G: Give the atom- and electron-balanced oxidation half-reaction occurring in acidic solution. Express your answer as a chemical equation. Include all phases. H: Give the atom- and electron-balanced reduction...
Knowing that the standard reduction potential, E half-cell is +0.34V of the Cu'jCu(s) (or knowing that...
Knowing that the standard reduction potential, E half-cell is +0.34V of the Cu'jCu(s) (or knowing that the standard oxidation potential, Eoo of the Cu(s)]Cu* or knowing that the standard oxidation potential, E )u half-cell is -0.34 V), what is the potential of the nickel half-cell? Is this Ed or E hat is the potential of the nickel half-cell? Is this E, or E. red 8. What is the standard reduction potential (SRP, Eond) of the Ni2 |Ni(s) halfcell? What is...
can anyone solve it ( half reaction method) oxidation -reduction equation .. can anyone do it...
can anyone solve it ( half reaction method) oxidation -reduction
equation .. can anyone do it neatly
PROBLEMS: Balance these equations 2. 3. Cu+HNO, → Cu(NQ), + No, + HO NaCl + HSO, + MnQ → Naso, + Mnso, + Ho + a, 6. (acidic) 7. (acidic) 8. (basic) Asor + l, → Asor + |- (basic) 10
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87...
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e - Sn2+ is +0.15...
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. 2H+ + 2e - H2 Fe3+ + 3e + Fe Sn2+ + 2e Fe2+ + 2e →...
9. What is the coefficient in front of H' when the half-reaction is correctly balanced in acidic solution (with low...
9. What is the coefficient in front of H' when the half-reaction is correctly balanced in acidic solution (with lowest whole-number coefficients)? NO," → NO A. 8 B.4 - C.3 D. 2 E. I 10. Which of the following best describes the following half-reaction involving the chromate ion after it is balanced in acidic solution (with lowest whole-number coefficients)? CrO2-(aq) → CrO2(8) A. 2 electron oxidation B. 2 electron reduction C. 3 electron oxidation D. 3 electron reduction E. 5...
What is the reduction half-reaction? In the electrolytic cell of this experiment, copper metal is the...
What is the reduction half-reaction? In the electrolytic cell of this experiment, copper metal is the anode and zinc metal the cathode. The electrolyte solution is sulfuric acid, H2SO4. Oxidation occurs at the copper anode, where Cu is oxidized to Cu^2+: Cu (s) → Cu^2+ (aq) + 2 e– During the experiment, you might have noticed that at the end of the trials, the solution becomes slightly blue, which proves the existence of aqueous Cu^2+. What is the reduction half-reaction...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq)...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq) → SO42- (aq) (ii) (acid solution) Pu(OH)4 (8) ► Pu+ (aq) (iii) (base solution) CN- (aq) → OCN- (aq) (iv) (base solution) RhO42- (aq) → Rh,03 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reactic Balance the following redox equations by the ion-electron half-reaction method: (a) (acid...
A chem igns a galvanic cell that uses these two half reactions: standard reduction potential half-reaction...
A chem igns a galvanic cell that uses these two half reactions: standard reduction potential half-reaction (aq)+4 H,0(1)+3e" → Cr(OH)2(3)+50H (aq) cro Ered=-0.13 V Fe?+ (aq)+e → Fe2+ (aq) E = +0.771 V Answer the following questions about this cell. 0-0 0 Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. X 5 Write a balanced equation for the overall reaction that powers the cell....
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Cr3+(aq) + 3e — Cr(s) Al(s)—+A13+(aq) + 3e (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. <> Submit Answer Retry Entire Group 9 more group attempts remaining When the following half reaction is balanced under acidic conditions, what are the coefficients of the species shown? NO3 + H —— NO + H2O In the above...
Knowing that the standard reduction potential, E half-cell is +0.34V of the Cu'jCu(s) (or knowing that the standard oxidation potential, Eoo of the Cu(s)]Cu* or knowing that the standard oxidation potential, E )u half-cell is -0.34 V), what is the potential of the nickel half-cell? Is this Ed or E hat is the potential of the nickel half-cell? Is this E, or E. red 8. What is the standard reduction potential (SRP, Eond) of the Ni2 |Ni(s) halfcell? What is...
can anyone solve it ( half reaction method) oxidation -reduction
equation .. can anyone do it neatly
PROBLEMS: Balance these equations 2. 3. Cu+HNO, → Cu(NQ), + No, + HO NaCl + HSO, + MnQ → Naso, + Mnso, + Ho + a, 6. (acidic) 7. (acidic) 8. (basic) Asor + l, → Asor + |- (basic) 10
Refer to this table of reduction potentials to answer the questions. Reduction half-reaction Potential (V) +2.87 Electrolytic cells use electricity to cause a nonspontaneous redox reaction to occur. An electrolytic cell is constructed using the following components: • a power source, such as a battery, • the substance that will undergo electrolysis, and • two inert electrodes (usually platinum), which serve as the electrical connection between the power source and the substance undergoing electrolysis. As with any cell, oxidation occurs...
Selective Oxidation The standard reduction potential for the half-reaction Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following cathodic half reactions would produce, at the anode, a spontaneous oxidation of Sn to Sn2+ but not Sn2+ to Sn4+. 2H+ + 2e - H2 Fe3+ + 3e + Fe Sn2+ + 2e Fe2+ + 2e →...
9. What is the coefficient in front of H' when the half-reaction is correctly balanced in acidic solution (with lowest whole-number coefficients)? NO," → NO A. 8 B.4 - C.3 D. 2 E. I 10. Which of the following best describes the following half-reaction involving the chromate ion after it is balanced in acidic solution (with lowest whole-number coefficients)? CrO2-(aq) → CrO2(8) A. 2 electron oxidation B. 2 electron reduction C. 3 electron oxidation D. 3 electron reduction E. 5...
1. (a) Balance the following half-reactions by the ion-electron half-reaction method: (i) (acid solution) HSO3- (aq) → SO42- (aq) (ii) (acid solution) Pu(OH)4 (8) ► Pu+ (aq) (iii) (base solution) CN- (aq) → OCN- (aq) (iv) (base solution) RhO42- (aq) → Rh,03 (s) (b) Which of the above equations are oxidation half-reactions? (c) Give the formulas of the reactants that become oxidized in the course of the reactic Balance the following redox equations by the ion-electron half-reaction method: (a) (acid...
A chem igns a galvanic cell that uses these two half reactions: standard reduction potential half-reaction (aq)+4 H,0(1)+3e" → Cr(OH)2(3)+50H (aq) cro Ered=-0.13 V Fe?+ (aq)+e → Fe2+ (aq) E = +0.771 V Answer the following questions about this cell. 0-0 0 Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. X 5 Write a balanced equation for the overall reaction that powers the cell....
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