Consider following half-cell reactions : Cu2+ + 2e– Cu Eº = 0.34 V Zn2+ + 2e– Zn Eº = – 0.76 V + 4H+ + 2e– SO2 + 2H2O Eº = 1.17 V Hence, select correct statement (s) : A Cu reacts with dil. H2SO4 forming H2 and SO2 B Cu reacts with concentrated H2SO4 forming SO2 C Zn reacts with concentrated H2SO4 forming SO2 D Both (2) and (3)
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Answer:
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Explanation:
The standard reduction potentials E
⊝
for the half reactions are follows :
Zn→Zn
2+
+2e
−
;E
⊝
=+0.76V
Fe→Fe
2+
+2e
−
;E
⊝
=0.41V
The EMF for the cell reaction Fe
2+
Zn→Zn
2+
+Fe is:
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ANSWER
Fe
2+
+Zn→Zn
2+
+Fe
Zn→Zn
2+
+2e
−
;E
⊝
=+0.76V
Fe→Fe
2+
+2e
−
;E
⊝
=+0.41V
These are oxidation potentials.
Reduction potentials are equal and opposite.
Fe forms cathode and Zn forms anode.
E
cell
⊝
=(E
red
⊝
)
c
+(E
oxid
⊝
)
a
= (-0.41 + 0.76) V
= 0.35 V
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