For the reagents below:- Write the redox half-reactions involved for each compound- Write the redox reactions involved between the two compounds, justifying the direction of the reaction (weconsider pH = 0).%3DFESO4 + KMNO4K2Cr2O7 + C2H5OHData (pH = 0):Redox coupleStandard electrode potentialE° (V)1,51Redox coupleStandard electrode potential E° (V)1,33MnO4- / Mn2+Fe3+ / Fe2+Cr20,2-/ Cr3*0,77CH3COOH / C2H5OH 0,15

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For the reagents below: - Write the redox half-reactions involved for each compound - Write the redox reactions involved between the two compounds, justifying the direction of the reaction (we consider pH = = 0). FeSO4 + KMNO4 K2Cr207 + C2H5OH Data (pH = 0): Redox couple Standard electrode potential E° (V) Redox couple Standard electrode potential E° (V) 151 1.33

For the reagents below: - Write the redox half-reactions involved for each compound - Write the redox reactions involved between the two compounds, justifying the direction of the reaction (we consider pH = = 0). FeSO4 + KMNO4 K2Cr207 + C2H5OH Data (pH = 0): Redox couple Standard electrode potential E° (V) Redox couple Standard electrode potential E° (V) 151 1.33

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter23: Potentiometry

Section: Chapter Questions

Problem 23.23QAP: The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300...

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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?
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Given the standard reduction potentials (Eo’) for ubiquinone (Q) and NADP+provided below, consider the following questions.Q + 2H+ + 2e- ---> QH2 Eo’ = 0.04 VNADP+ + H+ + 2e- ---> NADPH Eo’ = -0.32 V - Calculate the standard ΔEo’ for the oxidation of NADPH by Q. From the reactantsin your derived redox reaction, indicate the oxidant and reductant.- Calculate the standard free energy of the redox reaction in part (a) and indicate if thereaction is exergonic or endergonic.
Given a cell: 2 Ag+(aq) + Cu(s) ----> 2Ag (s) + Cu2+ (aq), E(cell) = 0.346 V, E0(cell) = E0cathode - E0anode = 0.800 V - 0.340 V = 0.460 V, I. calculate the concentration of Cu2+ given that of Ag+ is 1.0 x 10-5M Cu2+M= Keq =
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A glass / calomel electrode system was found to develop a potential of - 0.0412 V when used I a buffer of pH 6.00; with an unknown solution the potential was observed to be - 0.204 V. Calculate the pH and the [H+] of the unknown. The following cell was employed for the determination of pCrO4: SCE // CrO4 2-(xM) / Ag2CrO4 (s) / Ag (s) Find the pCrO4 if the cell potential is - 0.402 V (E0 Ag/Ag2CrO4 = - 0.316 V ; E SCE = 0.241 V)
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The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?
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