Electrode potential table

Chemically, it is clear that Zn and Cd are rather similar and that Hg is somewhat distinct. The lighter pair are more electropositive, as indicated both by their electronegativity coefficients and electrode potentials (Table 29.1), while Hg has a... 

The standard electrode potential of an element is defined as its electrical potential when it is in contact with a molar solution of its ions. For redox systems, the standard redox potential is that developed by a solution containing molar concentrations of both ionic forms. Any half-cell will be able to oxidize (i.e. accept electrons from) any other half-cell which has a lower electrode potential (Table 4.1). 

In the chart of standard electrode potentials (Table 12-1), reactions are arranged in order of their tendency to occur. Reactions with a positive EMF occur more readily than those with a negative EMF. The zinc-copper cell has an overall EMF of + 1.10 volts, so the solution of zinc and deposition of copper can proceed. 

Problem 38 Considering only the elements in the chart of standard electrode potentials (Table 12-2), which pair can make a battery with the greatest voltage What would the voltage be ... 

Electrode potentials for half-reactions are most easily obtained from a table of standard electrode potentials (Table 17-1, p 275) they may be modified for concentrations appreciably different from unit activity (p 276). A list of features characteristic of electron-transfer reactions is given on p 300. 

A second way of expressing the same information is to give electrode potentials (Table 6-8). Electrode potentials are also important in that their direct measurement sometimes provides an experimental approach to the study of oxidation-reduction reactions within cells. To measure an electrode potential it must be possible to reduce the oxidant of the couple by flow of electrons (Eq. 6-62) from an electrode surface, often of specially prepared platinum. 

Could (a) iron, (b) tin be substituted for zinc as the reducing agent in the chromous acetate preparation Give reasons for your answer, referring to a table of standard electrode potentials (Table 6, page 48). 

USES OF STANDARD ELECTRODE POTENTIALS Table 21-2 Standard Reduction Potentials in Aqueous Solution at 25°C... 

The standard free energy changes (AG ) can be determining by using standard electrode potentials. Table 19.4 summarizes the relationship between AG and E . 

Example 10.3 shows how an equilibrium constant may be computed using the standard electrode potentials. Table 10.1 lists some of the commonly used standard electrode potentials. In using the standard potentials, one must note that if the reaction is reversed, the sign of l o also reverses. 

The measure of the thermodynamic ease of reduction of a positive ion is the standard electrode potential (Table 16.1, page 325). Elements with very low s, therefore, are difBcult to prepare by the reduction of their salts. When the g" is lower than about —1.5 V, electrolytic reduction is used. An aqueous solvent must be avoided because water is more easily reduced and only gas would appear at the cathode. 

Like solubility products (page 344), these constants are calculated from standard electrode potentials (Table 22.3), Table 22.4 gives the dissociation constants of several complex ions. 

If, on the other hand, the substances taking part in the process are in their standard states, such that the activities of the metallic ions are equal to unity or gases are at 1 bar pressure, the potentials obtained are called Standard Electrode Potentials (Table 2.1). A standard potential refers to the potential of pure metal measured with reference to a hydrogen reference electrode. The details of reference electrodes are provided later in this chapter. 

Vi V 2 Standard half-cell electrode potentials (Table 17.1) for metals 1 and 2 (Reaction 17.17)... 

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