The 2nd picture is an example of Alex’s answer format 2+Ca(s) Ca²+ (aq) +2e2+• The reactant being reduced is zelectrons to form neutral zinc atodescribes this:2+Zn²+ (aq) +2eZn(S)Here is the completed table:EANSWER2+oxidation: Ca(s) → Ca“ (aq)+2e2+reduction: Zn(aq)+2eZn(s) O ELECTROCHEMISTRYWriting the half-reactions of a single-...Study this chemical reaction:AAoxidation:reduction:FeSO4(aq)+Zn(s) → Fe(S)+ZnSO4(aq)Then, write balanced half-reactions describing the oxidation and reduction thathappen in this reaction.ExplanationCheckローロwww-awa.aleks.come0/5Andrew?AoloArⒸ2023 McGraw HiIII LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

O ELECTROCHEMISTRY Writing the half-reactions of a single-... AA Study this chemical reaction: FeSO4(aq) +Zn(s) → Fe(S)+ZnSO4(aq) oxidation: reduction: Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. ローロ www-awa.aleks.com e 0/5 On Andre

O ELECTROCHEMISTRY Writing the half-reactions of a single-... AA Study this chemical reaction: FeSO4(aq) +Zn(s) → Fe(S)+ZnSO4(aq) oxidation: reduction: Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction. ローロ www-awa.aleks.com e 0/5 On Andre

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 14P

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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-.
An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
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.
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 a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?