Learning Goal:To learn how to use the Nernst equation.The standard reduction potentials listed in any reference table are only valid atthe common reference temperature of 25 °C and standard conditions of 1 Mfor solutions and 1 atm for gases. To calculate the cell potential at nonstandardconditions, one uses the Nernst equation,E=E 2.303 RT 1nF-log10 Qwhere E is the potential in volts. Eo is the standard potential at 25°C in volts.R 8.314 J/(K-mol) is the gas constant, T is the temperature in kelvins.12 is the number of moles of electrons transferred, F = 96, 500 C/(mol e-)is the Faraday constant, and is the reaction quotient.At the common reference temperture of 298 K. substituting each constant intothe equation the result isE = E-Vlog 10 Q0.0592 V71 What is the cell potential for the reactionat 49 °C when [Fe²+] = 3.80 M and [Mg²+] = 0.210 M.Express your answer to three significant figures and include the appropriate units.▸ View Available Hint(s)μAE= ValueSubmityUnitsMg(s) + Fe²+ (aq) →Mg²+ (aq) + Fe(s)?

In the given question we have to calculate the cell potential of the reaction, first of all, we…

What is the cell potential for the reaction at 49 °C when [Fe²+] = 3.80 M and [Mg²+] = 0.210 M. Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) μA E= Value Submit y Units Mg(s) + Fe²+ (aq) →Mg²+ (aq) + Fe(s) ?

What is the cell potential for the reaction at 49 °C when [Fe²+] = 3.80 M and [Mg²+] = 0.210 M. Express your answer to three significant figures and include the appropriate units. ▸ View Available Hint(s) μA E= Value Submit y Units Mg(s) + Fe²+ (aq) →Mg²+ (aq) + Fe(s) ?

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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A cell constructed in which one half-cell consists of a Zn wire dipped in a solution of Zn(NO3)2- The other half-cell is composed of an inert electrode in a solution containing a mixture of Fe and Fe* ions. What will the cell potential, Ecell, be if the soluble ions have the following concentrations at 25°C? [Zn**] = 0.49M; [Fe] = 0.16 M; [Fe*] = 0.41 M Draw the complete galvanic cell set-up for this. Label each component.
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Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs at 25.0∘C, given than [Ti2+] = 0.602 M and [Au3+] = 0.276 M. use standard reduction potentials
Using standard potentials given in the appendices, calculate the standard cell potentials for the following reaction: Cu(s) + 2Ag+ (aq) = Cu²+ + 2Ag(s) Report the answer in volts with three significant figures. 0.462 V Submit Previous Answers Correct Correct answer is shown. Your answer 0.46 V was either rounded differently or used a different number of significant figures than required for this part. Part B Determine the equilibrium constant for the above reaction.
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The following reaction occurs at 298 K: Zn(s) + 2Ag+(aq) --> Zn2+(aq) + 2Ag(s)Please help me calculate the potential of this cell when [Ag+] = 0.010M and [Zn2+] = 1.0 M.
+ Cell Potential and Equilibrium The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K FE RT where 72 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▾ Part A Use the table Express your answer numerically. ▸ View Available Hint(s) K= ΥΠΙ ΑΣΦ 9 Reduction half-reaction Ag+ (aq) +eAg(s) Cu²+ (aq) +201 >Cu(s) Sn+ (aq) + 4e →→Sn(s) 2H+ (aq) +2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe²+ (aq) + 2e →Fe(s) Zn²+ (aq) +2e →Zn(s) Al³+ (aq) + 3e →Al(s) Mg²+ (aq) + 2e →Mg(s) standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s) ? E (V) 0.80 0.34 0.15 0 0.26 -0.45 0.76 -1.66 2.37 29 o Review | Constants | Period
Part B Calculate the standard cell potential at 25 °C for the reaction X(s) + 2Y*(aq)–→X²+ (aq) + 2Y(s) where AH° = -593 kJ and AS° = -371 J/K Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? E° = |2,85 V Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining
An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 MNH3 that is also 0.0080M in Cu(NH3),+, what is the cell potential at 25°C? Cu?+ (ag) + 4 NH3 (aq) = Cu(NH3)4²* (aq) K = 1.0 × 1013 Cell potential V