When the Pb²+ concentration is 3.44×104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.137V. What is the Mg²+ concentration? Pb²+(aq) + Mg(s)- Answer: M Pb(s) + Mg²+ (aq)

When the Pb²+ concentration is 3.44×104 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.137V. What is the Mg²+ concentration? Pb²+(aq) + Mg(s)- Answer: M Pb(s) + Mg²+ (aq)

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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the standard cell potential (E°cell) for the voltaic cell based on the reaction below is what? Cr(s) + 3Fe3+(aq) --> 3Fe2+(aq) + Cr3+(aq)
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Determine the value of Ecell (25°C) for the following voltaic cell: GSW (s) ∣ GSW3+(aq, 0.389 M) ‖ GSW3+(aq, 1.15 M) ∣ GSW (s) +0.060 V +0.030 V -0.060 V -0.030 V -0.009 V +0.009 V 0.000 V
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+ 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