Based on these raw experimental data, calculate the Faraday constant. V(H2) = 41.1 ml; V(02) = 19.5 ml %3! P atm = 760.5 mmHg %3D Temperature = 27 °C Time of electrolysis: 46 min = 2769 seconds Current, i= 0.108 mA.

Consider a cell that uses the redox reaction: 3 Na (s) + La3+ (aq) → 3 Na+ (aq) + La (s). Calculate the equilibrium constant (K) for this reaction at 25 ºC, given the following standard reduction potentials: La3+ (aq) + 3 e- →  La (s)     E° = -2.37 V Na+ (aq) + e- → Na (s)         E° = -2.71 V       1.8 x 10-6     5.7 x 10-18     5.6 x 105     1.7 x 1017

29b

Standard Reduction Potentials at 25 °C Half-reaction. Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e →→Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Aut 2Au + Au³+ Will Au* disproportionate in aqueous solution? To justify your answer, what is the standard cell voltage for the disproportionation reaction?

Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an important biological reaction.Below are the reduction reactions and standard reduction potentials (E °) at pH = 7 and 25 ° C.Pyruvate + 2H + + 2e- = Lactate - (E ° = -0.185 V)Cytochrome C (Fe3 +) + e - = Cytochrome C (Fe2 +) (E ° = 0.254 V) Considering the Gibss free energy and Nernst equations, calculate the following equilibrium ratio (K) at 25 ° C, pH = 7.

Given the following information: • Electrochemical cell: Niº | Ni2+ || Ag+ | Ago • Half-cell reactions with corresponding Reduction Potential: o Ni2+ + 2e Niº ▪ °Ecell = -0.250 V o Ag++ 1e Agº ▪ °Ecell= + 0.800 V . Conditions: 1 molar concentrations for ions at at 25°C How many electrons were exchanged between the two cells? Please indicate your answer as a number (e.g. 15). N

Consider these two entries from a fictional table of standard reduction potentials. X+ (aq) + e¯ Y+ (aq) + e- →Y(s) E = 2.01 V →X(s) O X and Y O X+ and Y+ O X and Y+ O X+ and Y E = 2.62 V Which pair of species will react under standard conditions at 25 °C?

Standard Reduction Potentials (Volts) at 25 °C F2 (g) + 2 e-  2 F- (aq) 2.870 O2(g) + 4 H3O+(aq) + 4 e-  6 H2O(l)  1.229 2 H2O(l) + 2 e-  H2(g) + 2 OH-(aq) -0.828 Fe2+ (aq) + 2 e-  Fe (s) -0.440   A 0.122 M neutral aqueous FeF2 solution is electrolyzed under 1 atm pressure using platinum electrodes.(a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials.Half-reaction at anode:     +       +       ->       +       +     Half-reaction at cathode:     +       +       ->       +       +     (b) What is the expected decomposition potential? _______ V

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.