In acidic medium,dichromate ion oxidises ferr | vedclass

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(C) In acidic medium,the dichromate ion $(Cr_2O_7^{2-})$ acts as an oxidizing agent and is reduced to chromium$(III)$ ion $(Cr^{3+})$.The half-reactio

Vedclass · Accepted Answer

$49$

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(C) In acidic medium,the dichromate ion $(Cr_2O_7^{2-})$ acts as an oxidizing agent and is reduced to chromium$(III)$ ion $(Cr^{3+})$.The half-reaction is: $Cr_2O_7^{2-} + 14H^+ + 6e^- ightarrow 2Cr^{3+} + 7H_2O$.The change in oxidation state of chromium is from $+6$ to $+3$ for each $Cr$ atom. Since there are two $Cr$ atoms in $K_2Cr_2O_7$,the total change in oxidation state is $2 	imes (6 - 3) = 6$.Therefore,the $n$-factor for $K_2Cr_2O_7$ is $6$.The equivalent weight is calculated as: $	ext{Equivalent weight} = \frac{	ext{Molecular weight}}{n	ext{-factor}} = \frac{294}{6} = 49 \ g$.

In acidic medium,dichromate ion oxidises ferrous ion to ferric ion. If the gram molecular weight of potassium dichromate is $294 \ g$,its gram equivalent weight is $...$ grams.

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