3.) Consider that the following half reaction is assigned a half cell voltage of 0.00 V. Hg (aq) + 2 e ® Hg (I) E° = 0.00 V When this half-cell is paired with each of the following half-cells to form a complete cell in the laboratory, the following cell voltages are measured when the Hg cell is connected to the (+) terminal, thus acting as the cathode. Hg "Standard" Cell Potentials Ni/Ni2 with Hg/Hg. 1.134 V Sn/Sn2 with Hg/Hg. 0.99 V a. Calculate the reduction potentials using this Hg standard cell. Ni2 (aq) + 2 e ® Ni(s) V (Hg Standard) Sn-2 (aq) + 2 e Sn(s) V (Hg Standard)

3.) Consider that the following half reaction is assigned a half cell voltage of 0.00 V. Hg (aq) + 2 e ® Hg (I) E° = 0.00 V When this half-cell is paired with each of the following half-cells to form a complete cell in the laboratory, the following cell voltages are measured when the Hg cell is connected to the (+) terminal, thus acting as the cathode. Hg "Standard" Cell Potentials Ni/Ni2 with Hg/Hg. 1.134 V Sn/Sn2 with Hg/Hg. 0.99 V a. Calculate the reduction potentials using this Hg standard cell. Ni2 (aq) + 2 e ® Ni(s) V (Hg Standard) Sn-2 (aq) + 2 e Sn(s) V (Hg Standard)

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 100QAP: Consider the following standard reduction potentials:...

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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?
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-.
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.
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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, .
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
The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
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)
Consider the following standard reduction potentials: Tl+(aq)+eTl(s)Ered=0.34VTl3+(aq)+3eTl(s)Ered=0.74VTl3+(aq)+2eTl+(aq)Ered=1.28V and the following abbreviated cell notations: (1) Tl|Tl+Tl3+,Tl+|Pt (2) Tl|Tl3+Tl3+,Tl+|Pt (3) Tl|Tl+Tl3+|Tl (a) Write the overall equation for each cell. (b) Calculate E° for each cell. (c) Calculate G° for each overall equation. (d) Comment on whether G° and/or E° are state properties. (Hint: A state property is path-independent.)