Calculate the elecytomotive force (in volts) registered by an electrode immersed in a solution containing 8.13 mM NAD+ and 6.58 mM NADH+H at pH=7 and 250C, with reference to half-cell of E'0 0.00 V.
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- 1. Latimer diagrams for oxygen and iron under standard conditions are shown below. (a) Write down two balanced half-equations and an overall equation for the disproportionation of hydrogen peroxide to water and dioxygen and calculate the electrode potential (Eº) for this reaction. Is this reaction feasible (calculate Delta G)? (b) Calculate the skip-step potential for the reduction of O2 to H2O. (c) Are iron(II) salts primary chemical standards? (Hint: What happens whensolutions of iron(II) are exposed to air? You are required to determine anelectrode potential for this reaction).An electrochemical cell is constructed using 0.50 M NiSO4 and a solid nickel electrode in one half cell and 2.0 M ZnCl2 and a solid zinc electrode in the other half cell. The cell is run at 25oC. What voltage would be expected from this cell? Enter the response to 2 significant figures.Calculate the elecytomotive force (in volts) registered by an electrode immersed in a solution containing 3.55 mM NAD+ and 4.20 mM NADH+H at pH=7 and 25oC, with reference to half-cell of E'0 0.00 V.
- The specifications for a lead storage battery include delivery of steady 1.5 A of current for 15 h. Assume that the volume of the battery is 0.50L. what is the minimum concentration of H2SO4 necessary? Please answer with explanations(Please give clear handwritten answer) 0.1 M HNO3 solution at 298K was electrolyzed in Hittorf cell using platinum electrodes. After electrolysis, 34.2 mg of copper was deposited in coulometer which in series with the Hittorf cell. 50 mL of HNO3 solution was withdrawn from anode compartment after electrolysis and found to have a concentration of 0.0821 M. [Atomic mass Cu = 63]. (i) Find the transference number of H + and NO3 −. (ii) If 50 mL HNO3 solution was run off from cathode compartment, what would its concentration be?The following cell was found to have a potential of 0.124 V: Ag l AgCl(sat'd) ll Cu2+(0.00325 M) l membrane electrode for Cu2+When the solution of known copper activity was replaced with an unknown solution, the potential was found to be 0.086 V. Neglecting junction potential, what was the molar concentration of copper in this unknown solution?
- Hittorf cells with silver-silver chloride electrodes were filled with HCl solution with a molality of 0.0106 mol / kg. 2 mA strong current flowed into the cell for 3 hours. At the end of the experiment, the solution at the cathode contained 51.7169 g water and 0.0267 g HCl. Find the transport numbers H + and Cl-Calculate the cell potential of the lead dipole electrode when its concentration is (0.3) at a temperature of 25°C and after reducing it to single lead, its concentration becomes (0.6 M), knowing that the electromotive force is (v -0.126).(Give typed answer) How does li2O2 influence the secondary electrolyte interface in Li-ion battery?
- The cell Ag|AgCl(sat’d)||H+(a = x)|glass electrode has a potential of —0.2094 V when the solution in the right-hand compartment is a buffer of pH 4.006. The following potentials are obtained when the buffer is replaced with unknowns: (a) —0.2806 V and (b) —0.2132 V. Calculate the pH and the hydrogen ion activity of each unknown. (c) Assuming anuncertainty of 0.001 Vin the junction potential, what is the range of hydrogen ion activities withinwhich the true value might be expected to lie?I have tried using the Nernst equation but I keep getting the same wrong answer. How am I supposed to solve this? "Calculate the equilibrium potential of a copper wire immersed in 0.0003 M CuSO4 solution. The standard electrode potential for the reaction Cu2+ + 2e- = Cu0 at 25°C is 0.34 V (NHE). Now, answer the following questions. Calculate the ionic strength (M) of the solution. 1.2×10-3 Calculate the activity coefficient of Cu2+. 0.86 Calculate the equilibrium potential (v) of the copper wire electrode. Note: use activity instead of concentration."Nernst Equation A concentration cell is constructed of two hydrogen electrodes one immersed in a solution with H^+= 1.0 M and the other in 0.65 M KOH. c) Determine Ecell for the reaction that occurs. d) Compare this value of Ecell with E° for the reduction of H20 to H2(g) in basic solution, and explain the relationship between them.