Use a table to compare the similarities and differences between potentiometry, coulometry, and voltammetry. Consider the following comparisons: (a) The electrical measurement (e.g., current, potential, and charge), (b) The types of cells (galvanic and electrolytic), (c) The fundamental equation employed for quantitative measurement (Nernst, Faraday, and Ohm's), and (d) The ability for qualitative determination.

Use a table to compare the similarities and differences between potentiometry, coulometry, and voltammetry. Consider the following comparisons: (a) The electrical measurement (e.g., current, potential, and charge), (b) The types of cells (galvanic and electrolytic), (c) The fundamental equation employed for quantitative measurement (Nernst, Faraday, and Ohm's), and (d) The ability for qualitative determination.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter11: Dynamic Electrochemistry

Section: Chapter Questions

Problem 10P

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The table below lists the cell potentials for the 10 possible galvanic cells assembled from the metals A. B. C. D. and E. and their respective 1.00 M 2+ ions in solution. Using the data in the table, establish a standard reduction potential table similar to Table 17-1 in the text. Assign a reduction potential of 0.00 V to the half-reaction that falls in the middle of the series. You should get two different tables. Explain why, and discuss what you could do to determine which table is correct. A(s)in A2+(aq) B(s)in B2+(aq) C(s)in V2+(aq) D(s)in D2+(aq) E(s)in E2+(aq) 0.28V 0.81V 0.13V 1.00V D(s)in D2+(aq) 0.72V 0.19V 1.13V C(s)in V2+(aq) 0.41V 0.94V B(s)in B2+(aq) 0.53V
A cell was prepared by dipping a Cu wire and a saturated calomel electrode into 0.10 M CUSO4 solution. The Cu wire was attached to the positive terminal of a potentiometer and the calomel electrode was attached to the negative terminal. (a) Write a half-reaction for the Cu electrode. (b) Write the Nernst equation for the Cu electrode. (c) Calculate the cell voltage.
2. (a) A galvanic collis assembled using the AglAg' and AIJAP" olectrodes. Identify the cathode and the anode. Answers: (b) Write the balanced cell reaction for this cell. Answer: (c) Calculate the standard emf E" for this cell.
(a) The conductivity of 0.20 mol L-1 solution of KC1 is 2.48 X 10-2 S cm-1. Calculate its molar conductivity and degree of dissociation (a). Given X,°(K+) = 73.5 S cm2 mol-1 and Z°(cr) = 76.5 S cm2 mol-1.(b) What type of battery is mercury cell? Why is it more advantageous than dry cell?
What is the purpose of immersing the electrode in a saturated KCl solution? Is it proper to store the electrode in deionized water? Why or why not? Explain clearly and thoroughly.
A concentration cell was made using a Zn metal electrode in a saturated solution of ZNCO3 for the anode half cell, and a Zn metal electrode in 1.00 M Zn2* for the cathode half cell. E for the cell was 0.148 V at 25°C. Calculate the Ksp for ZnCO3. (Note: For purposes of this exercise, carry out the calculation to three significant figures.)
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I want Q3 (d) and (e)
(a) Determine the mass of Na,S2O3.5H20 required to prepare 0.1N solution in 50 ml volume. (b) Compare combustion of Anthracene and Xylene in sufficient supply of air. Which one will produce more carbon rich sooty flame and why? (c) Consider electrode potential data given in Question 4 (c). Predict which two electrodes combination will give maximum potential. Provide justification. (d) Explain two industrial applications of acidic buffer solutions. (e) Discuss the importance of Hess law with suitable example.
1.) A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction was 2H2O + H2+2OH^-. If a current of 3.0 amp was used for 30 min, what weight of H2O gas would be produced? 2.) What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in the electrolysis of H2O? 3.) Give the notation for the cell that utilizes the reaction: (a) Cl2 (g)+ 2 I^-(aq) to 2 Cl^-(aq)+I2(s), (b) what is the E^o for the cell? (c) which electrode is the cathode? 4.) The standard electrode potential fornthe Fe^2+ to Fe^(3+) + e - half reaction is -0.770V. (a) Using the Nernst equation [E=E^o - (0.059/n) log [Oxid]/[Red]]. Calculate the voltage of this half cell when the [Fe^3+] is 1.0 x 10^-3 and [Fe^2+] is 1.0 x 10 ^ -1. (b) Calculate the approximate equilibrium constant (K) for the half reaction.
3) Construct two electrochemical cells such that the EMF of the cells are less than +0.513 V. a. Before doing the simulation, predict the cells and explain. Justify using the Nernst equation. b. Provide the shorthand notation and EMF for each of the electrochemical cells that you construct.