Answer the following questions using data below the questions (all under standard conditions). a Is H2 (9) capable of reducing Ni²+(ag)? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E° (V) 2H* + 2e + H2 Ni2+ + 2e Ni -0.23 0.00 yes no b Will Sn+ oxidize Fe2+ to Fe+? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Sn+ + 2e + Sn2+ 0.15 Fe+ +e Fe²+ 0.77 yes no C Is Fe+ (g) capable of reducing VO2+(ag)? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Fe+ +e → Fe+ VO,+ + 2H+ + e + Vo2+ + H2O 0.77 1.00 yes no

Answer the following questions using data below the questions (all under standard conditions). a Is H2 (9) capable of reducing Ni²+(ag)? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E° (V) 2H* + 2e + H2 Ni2+ + 2e Ni -0.23 0.00 yes no b Will Sn+ oxidize Fe2+ to Fe+? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Sn+ + 2e + Sn2+ 0.15 Fe+ +e Fe²+ 0.77 yes no C Is Fe+ (g) capable of reducing VO2+(ag)? Assume that the reaction occurs at standard electrochemical conditions. Half-Reaction E (V) Fe+ +e → Fe+ VO,+ + 2H+ + e + Vo2+ + H2O 0.77 1.00 yes no

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter20: Chemistry Of Selected Transition Elements And Coordination Compounds

Section: Chapter Questions

Problem 107QRT: Repeat the directions for Question 106 using a cell constructed of a strip of nickel immersed in a...

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A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)
The equation G = nF also can be applied to half-reactions. Use standard reduction potentials to estimate Gf for Fe2+ (aq) and Fe3+ (aq). Gf for e= 0.)
Calculate the equilibrium constant for the following reactions using data from the standard reduction potential tables. (a) Cl2(g)+2Br-(aq)Br2(g)+2Cl-(aq) (b) Ni(s)+2Ag+(aq)2Ag(s)+Ni2+(aq) (c) I2(s)+Sn2+(aq)2I(aq)+Sn4+(aq)
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
Repeat the directions for Question 106 using a cell constructed of a strip of nickel immersed in a 1.0-M Ni2+ solution and a strip of silver dipping into a 1.0-M Ag+ solution. Write the balanced chemical equation for the reaction that is product-favored. Calculate the cell potential. Draw a sketch of the cell and indicate the anode, cathode, and direction of electron flow.
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.