Consider the following half-rHalAgSn2+A3+(1) The strongest oxidizing agent is:enter formula(2) The weakest oxidizing agent is:(3) The weakest reducing agent is:(4) The strongest reducing agent is:(5) Will Ag*(aq) oxidize Al(s) to Al(aq)?(6) Which species can be oxidized by Sn2*(aq)?If none, leave box blank.Submit AnswerTry Another Version1 item attempt remaining lm/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take[References]Use the References to access important values if needed for thConsider the following half-reactions:Half-reactionE° (V)Ag" (aq) + e-Ag(s) 0.799V2+Sn-"(aq) + 2e Sn(s) -0.140VAl3+"(аq) + Зе→ Al(s) -1.660V(1) The strongest oxidizing agent is:enter formula(2) The weakest oxidizing agent is:(3) The weakest reducing agent is:

Answered: Image /qna-images/answer/852f286f-fd11-4ed8-9e91-c6f6771d3fb4.jpg

Answered: enter formula 1) The strongest…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter22: Bulk Electrolysis: Electrogravimetry And Coulometry

Section: Chapter Questions

Problem 22.28QAP

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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-.
What cathode potential (versus SCE) would be required to lower the total Hg(II) concentration of the following solutions to 1.00 10-6 M (assume reaction product in each case is elemental Hg): (a) an aqueous solution of Hg2+? (b) a solution with an equilibrium SCN- concentration of 0.100 M? Hg2+ + 2SCN- Hg(SCN)2(aq) = Kf = 1.8 107 c) a solution with an equilibrium Br- concentration of 0.100 M? HgBr42++ 2e- Hg(l) + 4Br- E0= 0.223 V
Given the following: A cell SCE // Ag2CrO4 (saturated), CrO42- (xM) /AG is used for the determination of pCrO4- (ESCE = -0.244 V at 25 C). The half reaction at indicator electrode is: Ag2CrO4(s) + 2e-   2 Ag(s) + CrO42- (E0 = +0.446 V) What is pCrO4, given the cell potential of 0.402? What type of indicator electrode is Ag in this situation?
Which of the oxidizing agent listed is (are) capable of oxidizing Br - (aq) to BrO 3 - (aq) in acidicsolutions). Please answer with explanations. Thanks
ELECTROCHEMISTRY: Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X1 (where X is the anion) with a supplied current of 5.54 A for 11 h, consuming 0.1826 kWh of electrical energy. Assume that the current efficiency is 85%. (Input values only with 2 decimal places. Do not include the unit.)
The E°cell = 0.135 V for the reaction3I2(s) + 5Cr2O72-(aq) + 34H+(aq) → 6IO3-(aq) + 10Cr3+(aq) + 17H2OWhat is Ecell if [Cr2O72-] = 0.014 M, [H+] = 0.21 M, [IO3-] = 0.00018 M, and [Cr3+] = 0.0039 M?Ecell =
A 215 mL sample of a 0.500 M NaCl solution with an initial pHof 7.00 is subjected to electrolysis. After 15.0 minutes, a 10.0 mLportion (or aliquot) of the solution is removed from the cell andtitrated with 0.100 M HCl solution. The endpoint in the titrationis reached upon addition of 22.8 mL of HCl. Assuming constantcurrent, how much current (in A) was running through the cell?
The Zn-Cl battery has been suggested as an energy generator in transportation. The reactionis as follows:Zn (s) + Cl2 (g, 1 atm.) ZnCl2 (aq)a) It the molality of the electrolyte ZnCl2 is of 0.1 m, employ the Debye-Hückel law for calculating the average ionic activity coefficient (γ±), the average ionic activity (a±) and theelectrolyte’s activity (a2) b) Calculate the cell potential (Ecell), at 25 °C, using the values obtained in the previous section. Result a) γ±= 0.2768; a±=0.0440; a2=8.512 10-5 b) 2.2434 V
The following cell was used to determine the pSO4 of a solution: SCE||SO4^2-(Mx),Hg2SO4(sat'd)|Hg calculate the pSO4 if the cell potential was -0.474V.
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1.) A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction was 2H2O + H2+2OH^-. If a current of 3.0 amp was used for 30 min, what weight of H2O gas would be produced? 2.) What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in the electrolysis of H2O? 3.) Give the notation for the cell that utilizes the reaction: (a) Cl2 (g)+ 2 I^-(aq) to 2 Cl^-(aq)+I2(s), (b) what is the E^o for the cell? (c) which electrode is the cathode? 4.) The standard electrode potential fornthe Fe^2+ to Fe^(3+) + e - half reaction is -0.770V. (a) Using the Nernst equation [E=E^o - (0.059/n) log [Oxid]/[Red]]. Calculate the voltage of this half cell when the [Fe^3+] is 1.0 x 10^-3 and [Fe^2+] is 1.0 x 10 ^ -1. (b) Calculate the approximate equilibrium constant (K) for the half reaction.
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enter formula 1) The strongest oxidizing agent is: (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: