question_answer

Given, \[{{E}^{o}}_{C{{r}_{2}}O_{4}^{2-}/C{{r}^{3+}}}=1.34\,V,\,\,\,\,{{E}^{o}}_{Cl/C{{l}^{-}}}=\,\,1.37\,V\] \[{{E}^{o}}_{C{{u}^{3+}}/C{{u}^{+}}}=-\,0.74\,V,\,\,\,{{E}^{o}}_{MnO_{4}^{-}/M{{n}^{2+}}}=\,1.51\,\,V,\] Based on the data given above the strongest oxidizing agent will be

A) \[MnO_{4}^{-}\]         

B) \[M{{n}^{2+}}\]

C) \[C{{l}_{2}}\]              

D) \[C{{r}^{3+}}\]

Correct Answer: A

Solution :

[a] Most positive \[E{{{}^\circ }_{red}}/\] value means most oxidising agent Most negative \[E{{{}^\circ }_{red}}\] value means most reducing agent