When the Cu²+ concentration is 1.13 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 2.801 V. What is the Mg²+ concentration? Cu²+ (aq) + Mg(s) → Cu(s) + Mg²+ (aq) Cu²+ (aq) + 2e → Cu(s) E= 0.337 V Mg2+ (aq) + 2e → Mg(s) Ed=-2.370 V [Mg²+] = M

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)

When the Hg+ concentration is 1.44 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.717 V. What is the Zn2+ concentration? Hg (aq) + Zn(s) → Hg(1) + Zn²+ (aq) Zn M

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

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?

When the Pb²+ concentration is 1.14 M, the observed cell potential at 298 K for an electrochemical cell with the following reaction is 1.154 V. What is the Mn²+ concentration? 2+ Pb²+ (aq) + Mn(s) → Pb(s) + Mn²+ (aq) 2+ Pb²+ (aq) + 2e¯¯ → Pb(s) Fre (aq) + 2e¯ → Mn(s) E Mn²+ red 2+ Mn²+] = M -0.126 V -1.180 V

Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K.   Cd2+(aq) + 2e–   →  Cd(s)                     E° = –0.403 V                         Pb2+(aq) + 2e–   →   Pb(s)                     E° = –0.126 V     E°cell = ______________     Ecell = ______________

Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that [Cd²+] = 0.00100 M and [Au*] = 0.795 M. Standard reduction potentials can be found in this table. 3 Cd(s) + 2 Au³+(aq) =3 Ca²*(aq) + 2 Au(s) 1.81 E = Incorrect

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