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

The correct answer is "+2.37 V".

Step-by-step 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`