Two half cell reactions of an electrochemical cell are given below :
MnO–4(aq) + 8H+ (aq) + 5e– → Mn2+ (aq) + 4H2O (I), E° = + 1.51 V
Sn2+ (aq) → 4 Sn4+ (aq) + 2e–, E° = + 0.15 V
Construct the redox equation from the two half cell reactions and predict if this reaction favours formation of reactants or product shown in the equation...
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12th
Chemistry
Electrochemistry
Galvanic Cells
Two half - reaction of an e...
CHEMISTRY
Two half-reaction of an electrochemical cell are given below :
MnO
4
−
(aq)+8H
+
+5e
−
→Mn
2+
(aq)+4H
2
O(l);E
∘
=+1.51V
Sn
2+
(aq)→Sn
4+
(aq)+2e
−
,E
∘
=+0.15V
Construct the redox equation from the standard potential of the cell and predict if the reaction is reactant favoured or product favoured .
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ANSWER
At anode : [Sn
2+
(aq) → Sn
4+
(aq)+2e
−
]×5
At cathode : [MnO
4
−
(aq)+8H
+
(aq)+5e
−
→ Mn
2+
(aq)+4H
2
O(l)]×2
Cell reaction :
_____________________________________________________________________
2MnO
4
−
(aq)+5Sn
2+
(aq)+16H
+
(aq)→2Mn
2+
(aq)+5Sn
4+
(aq)+8H
2
O(l)
______________________________________________________________________
E
cell
∘
=E
cathode
∘
−E
anode
∘
=1.51V−0.15V
=1.36V
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