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 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)
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
Given the following two half-reactions in basic solutions, determine which overall reaction is spontaneous and calculate the cell potential. Draw an actual Galvanic cell, showing electron flow, ion flow, cathode, and anode. Write the shorthand standard cell notation. Br2(l) + 2 e- → 2 Br- (aq) E° = 1.07 V Cr3+(aq) + 3 e- → Cr(s) E°= -0.74 V
›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 (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. Excell 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?
Balance the following reaction. Calculate the cell potential and the Gibbs free energy of the reaction at standard conditions. Write the line representations for the Galvanic cells, indicating the anode and cathode.
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Given that the standard cell potential is 0.019 V and the overall equation is 2 Cr³⁺ (aq) + 3 Zn (s) → 2 Cr (s) + 3 Zn²⁺ (aq), what is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0323 M and [Cr³⁺] = 0.1736 M?
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…

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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