6D.4 The potential of the cell Pt(s)|H,(g,p®)[HCI(aq,b)|Hg,Cl,(s)|Hg(1) hasbeen measured with high precision with the following results at 25°C:b/(mmolkg") 1.60775.04033.07697.693810.9474E/V0.600 800.568 25 0.543 66 0.522 670.505 32Determine the standard cell potential and the mean activity coefficient of HCIat these molalities. (Make a least-squares fit of the data to the best straight line.)

The given cell reaction is Pt (s) │H2 (aq)│HCl (aq)│Hg2Cl2 (s)│ Hg (l) The Nernst equation is

Answered: 6D.4 The potential of the cell…

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 103CP

See similar textbooks

Similar questions

For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
Table 17-1 lists common half-reactions along with the standard reduction potential associated with each half-reaction. These standard reduction potentials are all relative to some standard. What is the standard (zero point)? lf is positive for a half-reaction, what does it mean? If is negative for a half-reaction, what does it mean? Which species in Table 17-1 is most easily reduced? Least easily reduced? The reverse of the half-reactions in Table 17-1 are the oxidation half-reactions. How are standard oxidation potentials determined? In Table 17-1, which species is the best reducing agent? The worst reducing agent? To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell)? Standard reduction and oxidation potentials are intensive. What does this mean? Summarize how line notation is used to describe galvanic cells.
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-.
From the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.
Calculate the standard potential of the cell Hg(l)|HgCI2(aq)||TINO3(aq)|TI(s) at 25 °C. (b) Calculate the cell potential when the molar concentration of the Hg2+ ion is 0.230 mol dm-3 and that of the Tl+ ion is 0. 720 mol dm-3.
Determine the emf for the cell Ag (s) | AgCl (s) | HCl (a = 1) | Cl2 (1 atm) | Pt given that the standard electrode potential of the Ag (s) | AgCl (s) | Cl- (aq) electrode is 0.2225 V, and that of the Pt | Cl2 (g) | Cl- (aq) is 1.3595 V.[1.137] The answer is written in the bracket. I would like to know how it is obtained. Thank you!
Consider the following electrochemical cell: Pt|H,(8,p°)|HCI(aq,b)|Hg.Cl,(s)|Hg() The potential of this cell, in relation to different molalities (b), has been measured with high precision at 25°C. The following results have been obtained: b/mmol.kg E/V I (ionic strength) Y: (DHLL) |Y: (linear fit) 1.6077 3.0769 5.0403 7.6938 10.9474 0.60080 0.56825 0.54366 0.52267 0.50532 (i) Write the half-reactions for the cell, and show the standard potential of each half-reaction. (ii) Determine the standard cell potential through simple calculation.
The galvanic cell Zn(s) | Zn2+(aq) | | Ni2+(aq)| Ni(s) is constructed using a completely immersed zinc electrode that weighs 32.68 g and a nickel electrode immersed in 575 mL of 1.00 M Ni2+(aq) solution. A steady current of 0.0715 A is drawn from the cell as the electrons move from the zinc electrode to the nickel electrode.(a) Which reactant is the limiting reactant in this cell?(b) How long does it take for the cell to be completely discharged?(c) How much mass has the nickel electrode gained when the cell is completely discharged?(d) What is the concentration of the Ni2+(aq) when the cell is completely discharged?
In the temperature range 0-90 ºC , the potential difference of the following cell: Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s) changes as follows with the temperature: Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.
In the temperature range 0-90 ºC , the potential difference of the following cell:Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s)changes as follows with the temperature:Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.Result: -34388 J/mol, 10.94 J/Kmol, -30.42 KJ/mol

Recommended textbooks for you

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

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

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:

9781305079113

Author:

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

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Physical Chemistry

Chemistry

ISBN:

9781133958437

Author:

Ball, David W. (david Warren), BAER, Tomas

Publisher:

Wadsworth Cengage Learning,

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

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

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS