Part 1: What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is 5.12x10-3 atm, the H+ concentration is 1.16M, and the Mn2+ concentration is 9.12×10-4M ? 2H+(aq) + Mn(s)→→→→ H₂(g) + Mn²+(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Part 2: V What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.05 atm, the F concentration is 1.25x10- 3M, and the Co2+ concentration is 1.64x10-4M ? F₂(g) + Co(s) 2F (aq) + Co²+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

Part 1: What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H₂ pressure is 5.12x10-3 atm, the H+ concentration is 1.16M, and the Mn2+ concentration is 9.12×10-4M ? 2H+(aq) + Mn(s)→→→→ H₂(g) + Mn²+(aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Part 2: V What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.05 atm, the F concentration is 1.25x10- 3M, and the Co2+ concentration is 1.64x10-4M ? F₂(g) + Co(s) 2F (aq) + Co²+ (aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:

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

See similar textbooks

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.
The following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
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+
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