Redox Reactions And Electrochemistry Ques 334

Question: The standard potential at 298 K for the following half reactions are given against each:

$ Z{n^{2+}}(aq)+2{e^{-}}\rightarrow Zn(s) $ $ -,0.762V $ $ 2{H^{+}}(aq)+2{e^{-}}\rightarrow H_2(g) $ 0.000 V $ C{r^{3+}}(aq)+3{e^{-}}\rightarrow Cr(s) $ $ -,0.740V $ $ F{e^{3+}}(aq)+2{e^{-}}\rightarrow F{e^{2+}}(aq) $ 0.770 V Which is the strongest reducing agent-

Options:

A) Zn(s)

B) Cr(s)

C) $ H_2( g ) $

D) $ F{e^{2+}}( aq ) $

Show Answer

Answer:

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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