A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e → NO(g) + 2H₂O (1) EO red = +0.96 V Cu2+ (aq) + e→ Cu+ (aq) EO red = +0.153 V The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] V.

A certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.00 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 anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? Data O yes, there is a minimum. E red = v 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. O no minimum Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is naximum. Pred = Iv 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. no maximum By using the information…

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Which of the following terms best describes the electrochemical reaction as written below.2 Pb 2+ ( aq) + 3 Au ( s) → 2 Pb ( s) + 3 Au 3+ ( aq)Standard Reduction PotentialsPb 2+ ( aq) + 2 e - → Pb ( s)   -0.13 VAu 3+ ( aq) + 3 e - → Au ( s)   1.50 V     The reaction is spontaneous.     The reaction is not spontaneous.     The spontaneity cannot be determined.

Consider the following electrochemical cell in which X is an unknown metal:       Pt (s) | Cl–(1 M) | Cl2 (1 atm) || X2+(1 M) | X (s)If the standard cell emf is 0.23 V, what is the standard reduction potential at 25○C for X2++ 2 e– → X (s)

A galvanic cell is powered by the following redox reaction: 3 Br,(1) + 2 MnO 2(s) + 8 OH (aq) → 6 Br (aq) + 2 MnO¿(aq) + 4 H,O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. e Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E = Iv Round your answer to 2 decimal places.

In the following: Al³+ (aq) + 3e → Al(s) E° = -1.66 V Cr³+ (aq) + 3e → Cr(s) E° = -0.74 V What is the standard cell potential for the corresponding galvanic cell? 0.00 V O-0.92 V +2.40 V +0.92 V O-2.40 V

A galvanic cell is represented by the shorthand Cu | Cu²⁺ || Ag⁺ | Ag. Which reaction occurs at the anode? A) Cu(s) → Cu²⁺(aq) + 2e⁻ B) Ag⁺(aq) + e⁻ → Ag(s) C) Cu²⁺(aq) + 2e⁻ → Cu(s) D) Ag(s) → Ag⁺(aq) + e⁻

|| Using the Nernst equation to calculate nonstandard cell voltage A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 0 2+ 2+ Cu (aq) + Zn (s) → Cu (s) + Zn²+ (aq) 2+ 2+ Suppose the cell is prepared with 1.39 M Cu in one half-cell and 2.14 M Zn in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. 0 x10 ロ・ロ X μ

Use the tabulated half-cell potentials to calculate the standard cell potential for the following balanced redox reaction. 312(s)+2 Fe(s) → 2 Fe3+(aq) +61 (aq) 12(s)+2e 21-(aq) E°=+0.54 V Fe3+(aq) +3 e → Fe(s) E°=-0.04 V A) +0.29 V B) +0.50 V C) -0.50 V D) -0.58 V E) +0.58 V