Consider the electrochemical cell, Ni (s) | NiCl2 (aq, 0.0050 mol kg − 1) | Hg2Cl2 (s) | Hg (l), for which Eo (Ni (s) / Ni2 + (aq)) = -0.257 V and Eo (Hg2Cl2 (s) / Hg (l)) = 0.268 V. A. Identify the balanced half-reactions of reduction and oxidation, b. Calculate the average ionic activity coefficient of NiCl2 from the limit law of Debye-Hückel. vs. Calculate the potential of the electrochemical cell, (2) d. Calculate ΔrG, ΔrGo, and K for the reaction of the electrochemical cell, (3) e. Given that (∂Ecell / ∂T) p = −4.52 × 10−4 V K − 1, calculate ΔrSo and ΔrHo.

Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C, given that 'Ce'[Sn'2] - 0.0652-text M[Sn²+] = 0.0652 M, 'Ce'[Co'3] - 0.0409-text M[Co³+] = 0.0409 M, 'Ce'[Sn'4] - 0.00496 'text' [Sn+] = 0.00496 M, and "C.[Co'2] - 0.01150 'text'[Co²+] = 0.01150 M. Standard reduction potentials can be found in this table. Sn²+(so much) + 2 Co³* (so much) = Sn* "(so much) + 2C0²+ (so much) E = V

The half-cell potential for the reactionO2 (g)+ 4H+ (aq) 4e → 2H2O (l)is 1.03V at 310K when activities of O2 and H2O are equal 1. What is the pH of this solution?

For the galvanic (voltaic) cell Fe(s) + Mn²⁺(aq) ⟶ Fe²⁺(aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²⁺] if [Mn²⁺] = 0.030 M and E = 0.78 V? Assume T is 298 K

Prepare a sketch and write the half-reactions and overall cell reaction for the electrochemical cell designated by:       Pt(s) | Ag(s) |AgCl(s) | Cl-(a = 1) | Cl2(g, 1 bar)| C(graphite) | Pt(s)

11-please see attached

Part A The following galvanic cell has a potential of 1.214 V at 25 °C: Hg(1)|Hg₂Br₂ (s)|Br¯(0.10 M)||MnO4¯ (0.10 M), Mn²+ (0.10 M), H+(0.10 M)|Pt(s) Calculate the value of Ksp for Hg₂Br₂ at 25 °C. Express your answer using one significant figure. Ksp = Submit 17 ΑΣΦ Request Answer ?

An aqueous LaI3 solution is electrolyzed under 1 bar pressure using platinum electrodes.(a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell potentials given below. Standard Reduction Potentials (Volts) at 25 °C I2(s) + 2 e-  2 I-(aq) 0.535 O2(g) + 4 H3O+(aq) + 4 e-  6 H2O(l) 1.229 2 H2O(l) + 2 e-  H2(g) + 2 OH-(aq) -0.828 La3+(aq) + 3 e-  La(s) -2.370 Half-reaction at anode:     +       +              +       +     Half-reaction at cathode:     +       +              +       +     (b) What is the expected decomposition potential?  _______V

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