12 In the electrolysis of an aqueous solution of AgBr, what are the products produced (use the following data; select ALL correct answers)?Reduction half reactionEred (V)2.87F2+2 e2F104+ 2 H+ 2 e 103 + H₂O1.60Cl₂ + 2 e2 ct1.36O₂ + 4H+4 e 2 H₂O1.23Br₂+2 e 2 Br1.07AgeAg0.8012+2 e210.53Cu²+ + 2 e→→ Cu0.34Ni²+ + 2 e→→ Ni-0.25Fe²+ + 2e →→ Fe-0.442 H₂O + 2 e → H₂ + 2 OH™-0.83-1.66Al³+ + 3 e → AlMg2+ + 2 eMg-2.37Na + e→→→ Na-2.71Li + eLi-3.05A Ag is producedthe anodeB. Ag is produced at the cathodeC.Br2 is produced at the anodeD. Br2 is produced at the cathodeOE.O2 and H* are produced at the anodeOFO2 and H* are produced at the cathodeH2 and OH are produced at the anodeΠΗ.H2 and OH are produced at the cathode

In electrolysis, Anion moves toward anode and get oxidized while cathode moves toward cathode and…

<->21 e Cu e → Ni 2e → Fe 2 e Be H₂ + 2 OH™ 2 e Mg e → Na TIL s produced at the anode s produced at the cathode is produced at the anode is produced at the cathode and H* are produced at the anode and H* are produced at the cathode and OH are produced at the anode and OH are produced at the cathode 0.53 0.34 -0.25 -0.44 -0.83 -1.66 -2.37 -2.71 -3.05 Al

<->21 e Cu e → Ni 2e → Fe 2 e Be H₂ + 2 OH™ 2 e Mg e → Na TIL s produced at the anode s produced at the cathode is produced at the anode is produced at the cathode and H* are produced at the anode and H* are produced at the cathode and OH are produced at the anode and OH are produced at the cathode 0.53 0.34 -0.25 -0.44 -0.83 -1.66 -2.37 -2.71 -3.05 Al

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 78QAP

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An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, 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 gold ions (based on your calculations)?
Consider the electrolysis of water in the presence of very dilute H2SO4. What species is produced at the anode? Atthe cathode? What are the relative amounts of the speciesproduced at the two electrodes?
1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 seconds
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)
What is the standard cell potential you would obtain from a cell at 25C 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)?
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
From the information provided, use cell notation to describe the following systems: (a) In one half-cell, a solution of Pt(NO3)2 forms Pt metal, while in the other half-Cell, Cu metal goes into a.Cu(NO3)2 solution with all solute concentrations 1 M. (b) The cathode consists of a gold electrode in a 0.55 M Au(NO3)3 solution and the anode is a magnesium electrode in 0.75 M Mg(NO3)2 solution. (c) One half-cell consists of a silver electrode in a 1 M AgNO3 solution, and in the other half-cell, a copper Electrode in 1 M Cu(NO3)2 is oxidized.
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
Use the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the reaction proceeds spontaneously as written or spontaneously in the reverse direction under standard-state conditions. (a) H2(g)+Cl2(g)2H+(aq)+2Cl(aq) (b) Al3+(aq)+3Cr2+(aq)Al(s)+3Cr3+(aq) (c) Fe2+(aq)+Ag+(aq)Fe3+(aq)+Ag(s)

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