Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for thefollowing balanced redox reaction at 25°C.2 Al(s) + 3 Mg²+(aq) → 2 Al3+(aq) + 3 Mg(s)4.6E+319.0E-731.0E+241.1E+721.1E-72

To calculate the equilibrium constant K for the given redox reaction, we need to use the Nernst…

Answered: Use the tabulated half-cell potentials…

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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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) Pb( s) + Br 2( l) → Pb 2+( aq) + 2 Br⁻( aq) Pb2+(aq) + 2 e⁻ → Pb(s) E° = -0.13 V Br2(l) + 2 e- → 2 Br-(aq) E° = +1.07 V
Calculate E°cell for the cell for the reaction 2 Ga(s) + 3 Sn4+(aq) → 3 Sn2+(aq) +2 Ga3+(aq).The standard reduction potentials are as follows: Ga3+(aq) + 3 e− → Ga(s) E° = –0.55 V Sn4+(aq) + 2 e− → Sn2+(aq) E° = 0.15V
›Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.867 M and [Fe²+] = 0.0100 M. Use the standard reduction potentials in this table. Zn(s) + Fe²+(aq) ⇒ Zn²¹(aq) + Fe(s) E = V
Use the hypothetical standard half-cell potentials listed below to calculate the standard cell potential in units of V for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)3 Cl 2(g) + 2 Fe(s) → 6 Cl⁻(aq) + 2 Fe 3+(aq)Cl 2(g) + 2 e⁻ → 2 Cl⁻(aq) E° = +1.73 VFe 3+(aq) + 3 e⁻ → Fe(s) E° = - 0.14 V
A galvanic cell is powered by the following redox reaction: MnO (aq) + 8H(aq) + 5 Cu* (aq) (aq) + 4H₂O(1) + 5 Cu²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. - Mn²+ ローロ X 00 3
Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)Mg2+(aq) + 2 e⁻ → Mg(s) E° = -2.37 VAl3+(aq) + 3 e⁻ → Al(s) E° = -1.66 V A) 1.0 × 1024 B) 1.1 × 10-73 C) 1.1 × 1072 D) 8.9 × 10-73 E) 4.6 × 1031
What is the standard cell potential for a galvanic cell made up of Ni and Zn?
red A certain half-reaction has a standard reduction potential E = +0.16 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…
Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +
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A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu²+ (aq) + 2Al(s) → 3Cu (s) +2A1³+ (aq) 2+ Suppose the cell is prepared with 4.04 M Cu²+ in one half-cell and 4.43 M A1³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 X 3 8 Ś

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Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg²+(aq) → 2 Al3+(aq) + 3 Mg(s) 4.6E+31 9.0E-73 1.0E+24 1.1E+72 1.1E-72