(C) The reduction half-reaction for the dichromate ion in an acidic medium is given by:$Cr_2O_7^{2-} + 14 H^+ + 6 e^- \rightarrow 2 Cr^{3+} + 7 H_2O$I

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(C) The reduction half-reaction for the dichromate ion in an acidic medium is given by:$Cr_2O_7^{2-} + 14 H^+ + 6 e^- \rightarrow 2 Cr^{3+} + 7 H_2O$In this reaction,the oxidation state of $Cr$ changes from $+6$ to $+3$.Since there are two $Cr$ atoms in $Cr_2O_7^{2-}$,the total change in oxidation state is $2 \times (6 - 3) = 6$.Therefore,$6$ electrons are required to reduce $Cr_2O_7^{2-}$ to $2 Cr^{3+}$.

Class 11 Chemistry Redox Reactions Redox reaction and Method for balancing Redox reaction

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The number of electrons required to reduce chromium completely in $Cr_2O_7^{2-}$ to $Cr^{3+}$ in acidic medium is:

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A
$5$
B
$3$
C
$6$
D
$2$

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Redox reaction and Method for balancing Redox reaction

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The number of electrons required to reduce chromium completely in $Cr_2O_7^{2-}$ to $Cr^{3+}$ in acidic medium is:

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$Na_2S_2O_3$ reacts with moist $Cl_2$ to form $Na_2SO_4$,$HCl$,and $X$. Which one of the following is $X$?

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