(A) In the given redox reaction,the oxidation state of $Cr$ changes from $+6$ in $Cr_2O_7^{2-}$ to $+3$ in $Cr^{3+}$.Since the oxidation state of $Cr$

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(A) In the given redox reaction,the oxidation state of $Cr$ changes from $+6$ in $Cr_2O_7^{2-}$ to $+3$ in $Cr^{3+}$.Since the oxidation state of $Cr$ decreases,$Cr$ is reduced.The oxidation state of $I$ changes from $-1$ in $I^{-}$ to $0$ in $I_2$.Since the oxidation state of $I$ increases,$I$ is oxidized.Therefore,the element reduced is $Cr$.