| \[{{F}_{2}}(g)=2{{e}^{-}}\xrightarrow[{}]{{}}2{{F}^{-}}(aq);\]\[{{E}^{o}}=+\,2.85\,V\] |
| \[C{{l}_{2}}(g)+2{{e}^{-}}\xrightarrow[{}]{{}}2C{{l}^{-}}(aq);\]\[{{E}^{o}}=+\,1.36\,V\] |
| \[B{{r}_{2}}(l)+2{{e}^{-}}\xrightarrow[{}]{{}}2B{{r}^{-}}(aq);\]\[{{E}^{o}}=+1.06\,V\] |
| \[{{I}_{2}}(s)+2{{e}^{-}}\xrightarrow[{}]{{}}2{{I}^{-}}(aq);\]\[{{E}^{o}}=+0.53\,V\] |
A) \[{{F}_{2}}\]and \[{{I}^{-}}\]
B) \[B{{r}_{2}}\] and \[C{{l}^{-}}\]
C) \[C{{l}_{2}}\] and \[B{{r}^{-}}\]
D) \[C{{l}_{2}}\] and \[{{I}_{2}}\]
Correct Answer: A
Solution :
Higher the value of standard reduction potential, stronger will be the oxidising agent. Therefore, F2 will act as strongest oxidizing agent. Similarly lower the value of standard reduction potential, stronger will be the reducing agent. Therefore, \[{{\text{I}}^{-}}\]will act as strongest reducing agent.
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