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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.

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Cricetus

Answer:

The correct answer is "+2.37 V".

Explanation:

Given that,

Concentration of [tex]Mg^{2+}[/tex]

= 1.00 M

[tex]E^0 \ Mg^{2+}/Mg[/tex],

= -2.37 V

[tex]E^0 \ \mu^+/H_2[/tex],

= 0.00V

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

⇒ [tex]E^0 cell=E^cathode-E^0 anode[/tex]

By putting the values, we get

⇒            [tex]=0.00V-(-2.37 V)[/tex]

⇒            [tex]=+2.37 \ V[/tex]    

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