Question

On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidizing agent.
(${E^ \circ }$value $F{e^{ + 3}} | F{e^{ + 2}} = + 0.77V:{I_2}(s) | {I^-} = 0.54V:C{u^{ + 2}} = 0.34V:A{g^ + } | A{g^ - } = + 0.8V$)
A. $F{e^{ + 3}}$
B. ${I_2}(s)$
C. $C{u^{ + 2}}$
D. $A{g^ + }$

Answer 1

Redox potential is an amount of the tendency of a chemical species to obtain electrons from or lose electrons to an electrode and thus be reduced or get oxidized. Redox potential is measured in volts, or millivolts. Each species has its own basic redox potential.

Complete step by step solution:
Since higher the reduction potential , better it acts as the oxidizing agent. Now, the reduction potential decreases in the order as below:
$A{g^ + } | Ag( + 0.80V) > F{e^{3 + }} | F{e^{2 + }}( + 0.77V) > {I_2}(s) | {I^-} ( + 0.4V) > C{u^{2 + }} | C{u^ + }(0.34V)$
So according to the above oxidizing order $A{g^ + }$ is the strongest oxidizing agent.

So the correct answer is D.

Additional information:
In aqueous solutions, redox capacity is calculated as the tendency of the solution to either gain or lose electrons when it's far from the trade by using the creation of a new species. A solution with a better concession capability than the new species will have a propensity to benefit electrons from the latest new species (that is to be decreased by means of oxidizing of the new species) and an answer with a lower concession ability will be prone to lose electrons to the brand new species (that is To be oxidized when decreasing the brand new species). This is due to the absolute potentials which are next to impossible to correctly degree, reduction potentials are defined as the relative to a reference electrode. Reduction potentials of aqueous solutions are calculated through measuring the ability distinction among an inert sensing electrode which is in touch with the answer and a strong reference electrode which is related to the answer by way of a salt bridge.

Note: The basis for an electrochemical cell, like the galvanic cell, is all the time a redox reaction which can be broken down into two half-reactions: first is oxidation at anode (loss of electron) and second is reduction at cathode (gain of electron). The electricity is produced due to electric potential difference between two electrodes. This potential difference is formed as a result of the difference between individual potentials of the two metal electrodes and the electrolyte. It is the amount of reducing power of any element or compound.