Question

chemical cell are given below:
Mno (aq) + 8H*(aq) + 5e
Mn²+ (aq) + 4H2O(I), E° = +1.51 V
Sn2+ (aq) Sn 4+ (aq) + 2e", E = +0.15 V
Construct the redox reaction from the two half cell reactions and predict if th
formation of reactants or products shown in the equation.
ns. The redox reaction will be
2MnO (aq) + 16H*(aq) + 5Sn2+ (aq)
(aq) -
2Mn2+ (aq) + 5Sn"+ (aq) + 8H 0(1)
If the oxidation occurs on Sn2+/Sn4+ electrode,
ECathode
E°
= 1.51 V – 0.15 V = 0.36 V, i.e., it will be positive.
Hence, reaction will favour formation of products,
4. State the factors that influence the value of cell potential of the following cell:
Mg(s)[Mg2+(aq) || Agt(aq)|Ag(s)
s. The factors that influence the value of cell potential are concentration of Mg and
and temperature.
5. Can Ecell or A,Gº for cell reaction ever be equal to zero?
:. No, Ecell or A,Gº for cell reaction can never be zero.
AG° = - nFE°
E cell
Anode​

Answer 1

Answer:

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