ELECTROCHEMICAL Standard Potentials: About this Simulation CELLS Gary L. Bertrand Universi Missouri-Rolla ound Select Electrode on Left: Select Electrode on Right: Zinc Iron Select Solution on Left: Select Solution on Right: Zinc Nitrate Iron(I) Nitrate Concentration (moles/liter): Concentration (moles/liter): 0.0001 to 2.00 0.0001 to 2.00 0 05 Solution in Salt Bridge is 0 01 Problem: Calculate the expected voltage (E) of this cell. Check Answer What is the cell potential in volts of the given cell above?

ELECTROCHEMICAL Standard Potentials: About this Simulation CELLS Gary L. Bertrand Universi Missouri-Rolla ound Select Electrode on Left: Select Electrode on Right: Zinc Iron Select Solution on Left: Select Solution on Right: Zinc Nitrate Iron(I) Nitrate Concentration (moles/liter): Concentration (moles/liter): 0.0001 to 2.00 0.0001 to 2.00 0 05 Solution in Salt Bridge is 0 01 Problem: Calculate the expected voltage (E) of this cell. Check Answer What is the cell potential in volts of the given cell above?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Nernst Equation and Equilibrium Potentials This case willgulde you through the principles underlying diffusion potetials and electrochemical equilibrium. Questions 1. A sohution of 100 mmol/L KCI is separated from a solution of 10 mmol/L Ka by a membrane that Is very permeable to K lons, but impermeable to C lons. What are the magnitude and the direc- tion (sign) of the potential difference that will be generated across this membranet (Assume that 2.3 RT/F-60 mV.) Will the concentration of K in either solution change as a result of the process that generates this potential difference? 2 Irthe same solutions of KCl described in Question I are now separated by a membrane that is very permeable to Cr ions, but impermeable to K lons, what are the magnitude and the sign of the potential difference that is generated across the membrane?
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Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25∘C and standard conditions of 1 MM for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=E∘−(2.303RT/nF) log10Q where E is the potential in volts, E∘ is the standard potential at 25 ∘C in volts, R=8.314J/(K⋅mol) is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F=96,500C/(mol e−) is the Faraday constant, and Q is the reaction quotient. At the common reference temperture of 298 K, substituting each constant into the equation the result is E=E∘−(0.0592 V/n)log10Q a) Calculate the standard cell potential at 25 ∘C for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) b) What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 57 ∘C when [Fe2+]= 3.80 MM and [Mg2+]= 0.210 MM .
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Research and write a report on the use of zinc as a “sacrificial anode” to minimize the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K
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INTERACTIVE EXAMPLE Electroplating How long will it take to plate out 4.2 g Ni from aqueous Ni2+ with a current of 112.3 A? HOW DO WE GET THERE? What is the quantity of charge carried by these electrons (in C)?