Question

Which of the following statement is true regarding the given standard potential?

$A{g}^{+}+e^{-}\to Ag;E^0=+0.8VS{n}^{2+}+2e^{-}\to Sn;E^0=-0.14V$

• A. $Ag$ will reduce $S{n}^{2+}$
• B. $Sn$ will reduce $A{g}^{+}$
• C. $Ag$ metal is more vulnerable to oxidation than $Sn$
• D. $S{n}^{2+}$ will oxidise $Ag$ metal

Answer 1

The correct option is B $Sn$ will reduce $A{g}^{+}$

Standard reduction potentials (SRP) of the half cell electrodes are calculated and arranged in a series of increasing order which is known as electrochemical series.
The standard electrode potential of $H^{+}/H_2$ couple is zero.

Here, a negative $E^0$ signifies that it has high tendency to get oxidised and the redox couple is a stronger reducing agent than the $H^{+}/H_2$ couple.

A positive $E^0$ signifies that it has high tendency to get reduced and the redox couple is a stronger oxidising agent than the $H^{+}/H_2$ couple.

Here, $E^0$ value of $A{g}^{+}/Ag$ couple is higher so it have more oxidising power than $S{n}^{2+}/Sn$ couple.
Hence,
$A{g}^{+}$ will oxidise $Sn$
$Sn$ will reduce $A{g}^{+}$

Due to lower $E^0$ value of $S{n}^{2+}/Sn$ couple, $Sn$ will have high tendency to get oxidised. Thus, $Sn$ metal is more vulnerable to oxidation than $Ag$.

Thus, option (b) is correct.