In an acidic medium,the dichromate ion oxidiz | vedclass

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(C) In an acidic medium,$K_2Cr_2O_7$ acts as a strong oxidizing agent and is reduced to $Cr^{3+}$.The half-reaction is: $Cr_2O_7^{2-} + 14H^+ + 6e^- \

Vedclass · Accepted Answer

$49$

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(C) In an acidic medium,$K_2Cr_2O_7$ acts as a strong oxidizing agent and is reduced to $Cr^{3+}$.The half-reaction is: $Cr_2O_7^{2-} + 14H^+ + 6e^- 	o 2Cr^{3+} + 7H_2O$.The change in oxidation state of $Cr$ is from $+6$ to $+3$. Since there are two $Cr$ atoms,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 mass is calculated as: $	ext{Equivalent mass} = \frac{	ext{Molar mass}}{n	ext{-factor}} = \frac{294}{6} = 49$.

In an acidic medium,the dichromate ion oxidizes the ferrous ion to the ferric ion. If the molar mass of potassium dichromate is $294 \, g/mol$,what is its equivalent mass?

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