Enter electrons as e.Use smallest possible integer coefficients.If a box is not needed, leave it blank.A voltaic cell is constructed from a standard HgHg half cell (E°.= 0.855V) and a standard Co-Co half cell (E°red = -0.280V).The anode reaction is:The cathode reaction is:The spontaneous cell reaction is:The cell voltage isV.

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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 83AP

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Similar questions

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-.
Is it reasonable to conclude that a potential could be assigned to each half-cell in a voltaic cell, based on these data for three voltaic cells? Explain. Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s) cell potential=1.10 V Zn(s)|Zn2+(aq)||Ag+(aq)|Ag(s) cell potential=1.56 V Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s) cell potential=0.46 V
Suppose Ered for H+H2 were taken to be 0.300 V instead of 0.000 V. What would be (a) Eox for H2H+ ? (b) Ered for Br2Br ? (c) E for the cell in 34(c)? Compare your answer with that obtained in 34(c).
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, .
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?
Using data from Table 17-1, place the following in order of increasing strength as reducing agents (all under standard conditions). Cu+,F,H,H2O,I2,K

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If a box is not needed, leave it blank A voltaic cell is constructed from a standard HgHg half cell (E°.ed= 0.855V) and a standard Co-"|Co half cell (E°red = -0.280V). The anode reaction is: The cathode reaction is: The spontaneous cell reaction is: The cell voltage is V.