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Consider the standard potential of the f...

Consider the standard potential of the following cells,
(i)`Mg^(2+) +2e rarr Mg,E^@=-2.37V`
(ii)`Zn^(2+) + 2erarrZn,E^@ =-0.76V`
(iii)`Ni^(2+) +2e rarrNi,E^@=-0.25V`
(iv)`Fe^(3+) + 3e rarrFe, E_0=-0.04 V` find the strongest reducing agent :

A

`Mg^(2+)`

B

`Zn^(2+)`

C

`Fe^(3+)`

D

`Ni^(2+)`

Text Solution

Verified by Experts

The correct Answer is:
B
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The standard reduction potential at 290K for the following half reactions are, (i) Zn^(2+) +2e rarrZn(s),E^@ =-0.762 V (ii) Cr^(3+) +3e rarr Cr(s), E^@=-0.740 V (iii) 2H^+ 2e rarrH_2(g),E^@=-0.000V (iv) Fe^(3+) +e rarr Fe^2+,E^@=+0.77V Which it the strongest reducing agent :

The standard cell potential for the cell is , Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu [E^@ for Zn^(2+)//Zn=-0.76V, E^@ for Cu^(2+)//Cu=+0.34V]

Calculate the standard emf of the cell having the cell reaction. Zn(s) + Co^(2+) ( aq) rarr Zn^(2+) ( aq) + Co(s) E_(Zn//Zn^(2+)) ^(@) = 0.76V, E_(Co//Co^(2+))^(@) = 0.25V

If Mg^(2+) +2e rarrMg(s), E=-2.37 V, Cu^(2+) + 2e rarrCu(s),E=+0.34V then the emf of the cell Mg|Mg^(+2)||Cu^(2+)|Cu is :

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