Which of the following reactions is possible | vedclass

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(A) The anode is the electrode where oxidation occurs. Oxidation involves the loss of electrons.In option $A$,the reaction is $2Cr^{3+} + 7H_2O \right

Vedclass · Accepted Answer

$2Cr^{3+} + 7H_2O \rightarrow Cr_2O_7^{2-} + 14H^{+} + 6e^{-}$

Vedclass · Answer

(A) The anode is the electrode where oxidation occurs. Oxidation involves the loss of electrons.In option $A$,the reaction is $2Cr^{3+} + 7H_2O \rightarrow Cr_2O_7^{2-} + 14H^{+} + 6e^{-}$. Here,the oxidation state of $Cr$ increases from $+3$ to $+6$,and electrons are released,which represents an oxidation process.In option $B$,$F_2$ gains electrons to form $F^{-}$,which is a reduction process.In option $C$,$O_2$ gains electrons to form $H_2O$,which is also a reduction process.Therefore,the reaction in option $A$ is the only one that represents oxidation and is possible at the anode.

Which of the following reactions is possible at the anode?

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