Given the following reduction potential data. E° (V) 12+ 2e → 21 (aq) Nat(aq) + e→→ Na O2 + 4H*(aq) + 4e → 2H₂O(1) 2H₂O(1) + 2e ->> H2 + 20H (aq) 0.53 -2.71 E (V) 0.82 (non standard conditions, [H*] = 10-7 M) -0.41 (non standard conditions, [OH-] = 10¹7 M) An electric current is passed through an aqueous solution of 1 M sodium iodide, Nal. What is produced at the anode and cathode? A. Sodium at the cathode, iodine at the anode. B. Sodium at the anode, iodine at the cathode. C. Hydrogen at the cathode, iodine at the anode. D. Sodium at the cathode, oxygen at the anode. E. Hydrogen at the cathode, oxygen at the anode.

Given the following reduction potential data. E° (V) 12+ 2e → 21 (aq) Nat(aq) + e→→ Na O2 + 4H(aq) + 4e → 2H₂O(1) 2H₂O(1) + 2e ->> H2 + 20H (aq) 0.53 -2.71 E (V) 0.82 (non standard conditions, [H] = 10-7 M) -0.41 (non standard conditions, [OH-] = 10¹7 M) An electric current is passed through an aqueous solution of 1 M sodium iodide, Nal. What is produced at the anode and cathode? A. Sodium at the cathode, iodine at the anode. B. Sodium at the anode, iodine at the cathode. C. Hydrogen at the cathode, iodine at the anode. D. Sodium at the cathode, oxygen at the anode. E. Hydrogen at the cathode, oxygen at the anode.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.18QAP

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The Nernst equation allows determination of the cell potential for a galvanic cell at nonstandard conditions. Write out the Nernst equation. What are nonstandard conditions? What do , n, and Q stand for in the Nernst equation? What does the Nernst equation reduce to when a redox reaction is at equilibrium? What are the signs of G and when K 1? When K 1? When K = 1? Explain the following statement: determines spontaneity, while determines the equilibrium position. Under what conditions can you use to predict spontaneity?
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
For the following half-reaction, = 2.07 V: A1F63(aq)+3eAl(s)+6F(aq) Using data from Table 17-1, calculate the equilibrium constant at 25C for the reaction A13+(aq)+6F(aq)A1F63(aq)K=?
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 aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
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-.

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