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11 Nov 2019
(a) Describe carefully what is meant by the term standard electrode potential. Explain how tables of standard half-cell potentials can be produced. (b) An electrochemical cell is constructed from two half-cells: on the right a silver wire dips into a 0.001 mol dm^-3 AgNO_3 solution, and the half-cell on the left is a hydrogen electrode with hydrogen gas at 1 bar pressure and an HCl solution of variable concentration, m. At 298 K the cell potential was found to vary with m in the following way: Determine the Nernst equation for the cell and then, by plotting a suitable straight-line graph, test how well the above data fit your equation. (c) From your graph, estimate the standard half-cell potential of the Ag^+/Ag couple.
(a) Describe carefully what is meant by the term standard electrode potential. Explain how tables of standard half-cell potentials can be produced. (b) An electrochemical cell is constructed from two half-cells: on the right a silver wire dips into a 0.001 mol dm^-3 AgNO_3 solution, and the half-cell on the left is a hydrogen electrode with hydrogen gas at 1 bar pressure and an HCl solution of variable concentration, m. At 298 K the cell potential was found to vary with m in the following way: Determine the Nernst equation for the cell and then, by plotting a suitable straight-line graph, test how well the above data fit your equation. (c) From your graph, estimate the standard half-cell potential of the Ag^+/Ag couple.
Hubert KochLv2
12 Jul 2019