The cell potential of the following cell is determined using an unspecified concentration of acid. What is[H] given that the measured cell potential is -0.464 V and the anode reduction potential (E°) is 0.222 Vat 25°C?Ag(s) | AgCl(s) | CI"(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s)O a) 9x 10-3 MO b) 9.3 x 10-6 MC) 2.6 x 10-12 MO d) 6.7x 10-9 MO e) 8.2 x 10-5 M

Anode half cell reaction: Cathode Half reaction: Overall reaction taking place is as follows:

Answered: The cell potential of the following…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 50QRT

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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.
Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
The standard potential, E, for the reaction of Zn(s) and Cl2(g) is +2.12 V. What is the standard free energy change, rG, for the reaction?
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 cell potential of the following cell is determined using an unspecified concentration of acid. What is [H*]given that the measured cell potential is -0.366 V and the anode reduction potential (E') is 0.222 V at 25°C? Agls) | AgCl(s) | CI(1.0 M) || H*(aq, ? M) | H2(g, 1.0 atm) | Pt(s) O 6.1x 102 M O 3.7 x 103M O 4.9x 105 M
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!
The cell notation of an electrochemical cell is given as below. Zn(s) |Zn²*(aq, 1.0 M)|| H*(aq, 1.0 M)|H,(g, 1 atm)|Pt(s) (a) Given that the cell potential is +0.76 V at 25°C, calculate the standard electrode potential for Zn*/Zn. (b) The cell potential of the above cell is recorded as +0.67 V at 25°C when hydrochloric acid and 1.0 atm hydrogen gas is used. Calculate the pH of the hydrochloric acid.
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A) For the concentration cell: Pt(s) | H2(g), H+(aq) (pH = 10) || H+(aq) (pH = 4), H2(g) | Pt(s), what is Ecell? B) For the concentration cell: Pt(s) | H2(g), H+(aq) (pH = 10) || H+(aq) (pH = 4), H2(g) | Pt(s), what is Ecell and the pH, when the cell attains equilibrium?
For the cell shown, the measured cell potential, Ecell, is -0.3621 V at 25 °C. Pt(s) | H₂(g, 0.765 atm) | H* (aq, ? M) || Cd² (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e Cd²+(aq) + 2 e H₂(g) + Cd(s) Calculate the H* concentration. [H+] = Eº = 0.00 V E° = -0.403 V M
A student decides to measure the solubility of lead sulfate in water and sets up the electrochemical cell Pb|PBSO4 |SO; (aq, 0.0500 M)||CI¯ (aq, 1.00 M)| AgCl|Ag At 25°C the student finds the cell potential to be 0.546 V, and from Appendix E the student finds AgCl(s) + ez Ag(s) + CI¯(aq) E° = 0.222 V What does he find for the Kp of PbSO4?
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