1. For the reaction: Cus) + 2Ag+ (aq) → 2+ Oxidation half-reaction: Cu(s) → Cuaq) + 2e¯ + Reduction half-reaction: 2Agaq) +2e → 2Ag Answer the following questions using Table 5.4.1: Table 5.4.1. Selected Standard Reduction Potentials at 25 °C Adapted from https://opentextb_c.ca/chemistry/chapter/17-3- Half-Reaction F2)+2 e2F¯(aq) O2(g) + 4H+ (aq) + 4e¯ → 2H₂O) Ag+(aq) + e → Ag(s) → Fe 2+ (aq) Fe³+ (aq) + e 12(1) + 2e™ 21 (24) Cu²+ (aq) + 2e Cu(s) - 2H*(aq) + 2e H₂0) + 2e → Zn(s) Zn² (29) Mg2 (aq) + 2 e→→ MgG) Ca²+ (aq) + 2e →→ Ca(s) a. What is the Eº of the anode half-cell? What is the Eº for the cathode half-cell? c. Calculate the Eᵒcell for the reaction. b. Cu²+ (aq) + 2Ag(s) standard-reduction-potentials/ E° (V) +2.87 +1.23 +0.80 +0.77 +0.54 +0.34 0.00 -0.76 -2.37 -2.87

1. For the reaction: Cus) + 2Ag+ (aq) → 2+ Oxidation half-reaction: Cu(s) → Cuaq) + 2e¯ + Reduction half-reaction: 2Agaq) +2e → 2Ag Answer the following questions using Table 5.4.1: Table 5.4.1. Selected Standard Reduction Potentials at 25 °C Adapted from https://opentextb_c.ca/chemistry/chapter/17-3- Half-Reaction F2)+2 e2F¯(aq) O2(g) + 4H+ (aq) + 4e¯ → 2H₂O) Ag+(aq) + e → Ag(s) → Fe 2+ (aq) Fe³+ (aq) + e 12(1) + 2e™ 21 (24) Cu²+ (aq) + 2e Cu(s) - 2H*(aq) + 2e H₂0) + 2e → Zn(s) Zn² (29) Mg2 (aq) + 2 e→→ MgG) Ca²+ (aq) + 2e →→ Ca(s) a. What is the Eº of the anode half-cell? What is the Eº for the cathode half-cell? c. Calculate the Eᵒcell for the reaction. b. Cu²+ (aq) + 2Ag(s) standard-reduction-potentials/ E° (V) +2.87 +1.23 +0.80 +0.77 +0.54 +0.34 0.00 -0.76 -2.37 -2.87

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 106QAP: In biological systems, acetate ion is converted to ethyl alcohol in a two-step process:...

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Calculate the standard potential for the half-reaction BiOCl(s)+2H++3eBi(s)+Cl+H2O given that Ksp for BiOCl has a value of 8.1 10-19.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(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-.
Consider a concentration cell that has both electrodes made of some metal M. Solution A in one compartment of the cell contains 1.0 M M2+. Solution B in the other cell compartment has a volume of 1.00 L. At the beginning of the experiment 0.0100 mole of M(NO3)2 and 0.0100 mole of Na2SO4 are dissolved in solution B (ignore volume changes), where the reaction M2+(aq)+SO42(aq)MSO4(s) occurs. For this reaction equilibrium is rapidly established, whereupon the cell potential is found to be 0.44 V at 25C. Assume that the process M2++2eM has a standard reduction potential of 0.31 V and that no other redox process occurs in the cell. Calculate the value of Ksp for MSO4(s) at 25C.
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.