11. Draw the following galvanic (voltaic) cells (salt bridge design) and label the following: i) anode and cathode ii) oxidation and reduction half reaction iii) direction of electron, cation and anion movement iv) net reaction v) calculate the E'cell a) Cou |Co(NO,)2 (aq) || Zn(NO3)2 (aq) | Zn (s) (standard conditions) b) Au(s) |Au(NO,); (aq) || H2(g), HCI (aq) | Pt (s) (hydrogen standard cell) c) Sn(s) |Sn(NO)2 (1.00 M) || Zn(NO)½ (0.0100 M) | Zn(s)

11. Draw the following galvanic (voltaic) cells (salt bridge design) and label the following: i) anode and cathode ii) oxidation and reduction half reaction iii) direction of electron, cation and anion movement iv) net reaction v) calculate the E'cell a) Cou |Co(NO,)2 (aq) || Zn(NO3)2 (aq) | Zn (s) (standard conditions) b) Au(s) |Au(NO,); (aq) || H2(g), HCI (aq) | Pt (s) (hydrogen standard cell) c) Sn(s) |Sn(NO)2 (1.00 M) || Zn(NO)½ (0.0100 M) | Zn(s)

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 76AP

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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-.
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 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 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)
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Consider a cell reaction at 25°C where n=4 . Fill in the following table.
Consider a cell reaction at 25°C where n=2 . Fill in the following table.
Calculate the theoretical potential of each of the following cells.Is the cell reaction spontaneous as written or spontaneous in the opposite direction? (a) Bi|BiO+ (0.0300 M),H+ (0.100 M)||I- (0.100 M), AgI(sat’d)|Ag (b) Zn|Zn2+(5.75 10-4M)||Fe(CN)64-(530 10-2 M),Fe(CN)63-(6.75 10-2M)|Pt (c) Pt,H2O (0.200 atm)|HCI(8.25 10-4M), AgCI(sat’d)| Ag
Consider a voltaic cell in which the following reaction takes place. 2F2+(aq)+H2O2(aq)+2H+(aq)2Fe3+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Calculate E at 25°C under the following conditions: [Fe2+]=0.00813M,[H2O2]=0.914M,[Fe3+]=0.199M,ph=2.88 .
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Consider a voltaic cell at 25°C in which the following reaction takes place: MnO2(s)+4H+(aq)+2Br(aq)Br2(l)+Mn2+(aq)+2H2O (a) Calculate E°. (b) Write the Nernst equation for the cell. (c) Find E under the following conditions: [Mn2+]=0.60M,[Br]=0.83M,pH=3.71 .