Electrochemistry

The reduction potential for to is
It can oxidise only those metals, which have reduction potential lower than For and , reduction potential given is and respectively. These values are lower than reduction potential of
Hence, and Ag will be oxidised. Since, for , reduction potential is higher, hence it will not be oxidised by Mn.

Both the electrode potential and the reduction potential are referred to as the oxidation potential. If oxidation occurs at the electrode under these circumstances, An increase in electrons is a component of reduction. The reduction potential of an electrode is therefore defined as its propensity to create electrons. The electrode potential is the difference in equilibrium potential between a solution electrode and a metal electrode. It is also defined as an electrode's propensity to produce more and less electrons.

Calculating the individual's reversible electrode potential at the standard state with ions at an altered concentration of 1 mol dm-3 atmospheric pressure is an element (E°) in electrochemistry. The standard potential for reduction is then frequently expressed as the typical electrode potential. The standard reduction potential may be calculated by subtracting the standard reduction potential for the cathode reaction from the standard reduction potential for the reaction occurring at the anode. Put the cell potential together to obtain the smallest simple cell potential. A potential distinction is framed at the metal interface and the solution when a metal piece is Solutions in its own response particles. The amount of the potential difference is a function of the cathode's tendency to experience either an increase in oxidation or a reduction in oxidation, or its propensity to either lose or gain electrons. The answer is the half-reaction, and the particle and metal stand for the half-cell. An electrode is the flooded metal, and the potential resulted from a reaction at the electrode contact. The electrode potential is the term for the answer. Accordingly, the terminal potential is represented as the cathode's propensity to either lose or gain electrons.

The oxidation potential is referred to as a result of the oxidation occurring at the electrode centre.

Potential for oxidation minus that of reduction.

(we assume that standard emf of the cell is known) 
For the given equilibrium, 

At equilibrium, 

Hence, we can calculate the equilibrium constant for reaction as follows : 

Where, is unknown 

The largest potential difference between two electrodes of a cell, while no current is being pulled from the cell, is known as the electromotive force, or EMF. The charges in an electric circuit move, and in order for the charges in a specific electric circuit to move, we must apply an external force to that electric circuit.

A battery or any other possible difference-making mechanism can serve as the source of an external force. The electromotive force, which is applied by the external electric source and accelerates the charges, is a physical force. 

Considering the formula for electromotive force as,

ε = V + Ir

Where

• The voltage of the cell is V.
• Current across the circuit is I.
• The internal resistance of the cell is R.
• The electromotive force is ε.

Kp is the equilibrium constant determined from the partial pressure of the equation of a reaction. It's a mathematical expression to determine the relation between product and reactant pressures. Although it connects the pressures, it is a unitless number. 

Kc is the equilibrium constant for a reversible reaction, which depicts the ratio of the equilibrium concentrations of products over the concentrations of reactants, where each is raised to the power of their stoichiometric coefficients.