| The standard potential at 298 K for the following half reactions are given against each: |
| \[Z{{n}^{2+}}(aq)+2{{e}^{-}}\rightleftharpoons Zn(s)\] \[-\,0.762\text{ }V\] |
| \[2{{H}^{+}}(aq)+2{{e}^{-}}\rightleftharpoons {{H}_{2}}(g)\] 0.000 V |
| \[C{{r}^{3+}}(aq)+3{{e}^{-}}\rightleftharpoons Cr(s)\] \[-\,0.740\text{ }V\] |
| \[F{{e}^{3+}}(aq)+2{{e}^{-}}\rightleftharpoons F{{e}^{2+}}(aq)\] 0.770 V |
| Which is the strongest reducing agent? |
A) Zn(s)
B) Cr(s)
C) \[{{H}_{2}}\left( g \right)\]
D) \[F{{e}^{2+}}\left( aq \right)\]
Correct Answer: A
Solution :
[a] The more negative the standard potential, the least the reduction tendency of the ion. The corresponding atom has largest oxidation tendency and thus is a strong reducing agent. In the present case. Zn is the strongest reducing agent.
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