Question

A voltaic cell consists of a standard hydrogen electrode and a second half-cell in which a magnesium electrode is immersed in a 1.00 M solution of Mg2+ ions. Calculate Ecell given that the standard reduction potential for the magnesium half-reaction is -2.37 V.

Answer 1

Answer:

The correct answer is "+2.37 V".

Explanation:

Given that,

Concentration of $Mg^{2+}$

= 1.00 M

$E^0 \ Mg^{2+}/Mg$,

= -2.37 V

$E^0 \ \mu^+/H_2$,

= 0.00V

When S.H.E as well as anode act as cathode, then

⇒ $E^0 cell=E^cathode-E^0 anode$

By putting the values, we get

⇒            $=0.00V-(-2.37 V)$

⇒            $=+2.37 \ V$