Standard reduction potentials notation

Reduction Half-Cell Reaction Cell Notation Standard Reduction Potential, V... 

Table 7.1 Selected standard reduction potentials (at 298 K) further data are listed in Appendix 11. The concentration of each substance in aqueous solution is Imoldm and the pressure of a gaseous component is 1 bar (10 Pa). Note that where the halfcell contains [OH] , the value of E° refers to [OH ] = Imoldm , and the notation °[oh-] = i should be used (see Box 7.1).

To determine the standard cell potential for a redox reaction, the standard reduction potential is added to the standard oxidation potential. What must be true about this sum if the cell is to be spontaneous (produce a galvanic cell) Standard reduction and oxidation potentials are intensive. What does this mean Summarize how line notation is used to describe galvanic cells. 

You are given the half-cell equations and can find standard reduction potentials in Table 20.1. The half-reaction with the lower reduction potential will be an oxidation. With this information, you can write the overall cell reaction, calculate the standard cell potential, and describe the cell in cell notation. 

On the basis of the standard reduction potentials shown above, which standard cell notation correctly represents its voltaic cell ... 

CHEMICAL AND THEORETICAL BACKGROUND Box 8.1 Notation for standard reduction potentials... 

Some texts use the notation E for the standard oxidation-reduction potential. 

For example, for iron in aqueous electrolytes, the thermodynamie warning of the likelihood of corrosion is given by comparing the standard electrode potential of the metal oxidation, with the potential of possible reduetion reactions. The metal anodie oxidation reaction, Fe —> Fe + 2e , can be written in the standard (reduction) notation as ... 

From a table of electrode potentials, write the two reduction half-reactions and standard electrode potentials for the cell. The cell notation assumes that the anode (the oxidation half-cell) is on the left. Change the direction of this half-reaction and the sign of its electrode potential. (Assuming that the cell notation was written correctly, you change the direction of the half-reaction corresponding to the smaller, or more negative, electrode potential.) Multiply the half-reactions (but not the electrode potentials) by factors so that when the half-reactions are added, the electrons cancel. The sum of the half-reactions is the cell reaction. Add the electrode potentials to get the cell emf. 

In Appendix D, we have modified the table of Standard Electrode (Reduction) Potentials at 25 °C so that it now includes a column with the cell notation for the half-reactions. 

Describe the role of non-fVwork in electrochemical systems. Define the roles of the anode, cathode, and electrolyte in an electrochemical cell. Given shorthand notation for an electrochemical cell, identify the oxidation and reduction reactions. Use data for the standard half-cell potential for reduction reactions, E°, to calculate the standard potential of reaction E. Apply the Nernst equation to determine the potential in an electrochemical cell given a reaction and reactant concentrations. 

The reactant and product species for both the reduction half-reaction and the hydrogen oxidation half-reaction are specified to be in their standard states. Recall that the standard state of a gas is an ideal gas at 1 bar, a liquid is a 1 m ideal solution in the Henry s law sense, and a solid is the pure solid with an activity of 1. In terms of our shorthand notation, we can measure the standard potential of any reduction half-reaction with a standard hydrogen electrode (S.H.E.) ... 

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