construct the table of aluminum electrode potentials as a function of the concentration of Al3 + ions. These concentrations are taken to be 1; 0.1; 0.0001 and 0.00001 mol / liter. Based on this table construct the curve that expresses the dependence of the electrode potential on the concentration. The standard electrode potential of aluminum is -1.66 V

Q: Mg(s) + Fe2+(aq) – Mg2+(aq) + Fe(s) The galvanic cell described above has a standard cell potential…

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Q: Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations…

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Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

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Q: Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.41 V; Zn²+ (aq)…

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Q: Calculate the cell potential, ?, for the given reactions at 25.00 °C using the ion concentrations…

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Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

A: The expression of Nernst equation is shown below: Ecell = E0cell -0.0591nlog Q Where; Ecell= cell…

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Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at 25…

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Q: In a standard electrochemical cell, A4+ constant is 2.23x1054 (Use R = 8.314 J/mol-K; F = 96485…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.753 M and…

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Q: Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.36 V; Zn2+ (aq)|…

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Q: Using these metal ion/metal standard reduction potentials: Cd²+ (aq)| Cd(s): -0.38 V; Zn²+ (aq…

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Q: Ag(s) Pb(s) salt bridge True True Determine which of the following statements about the cell shown…

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Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

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