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

24.5

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49

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125

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250

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Solution

The correct option is D $49$
$C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 F e^{2 +} \to 2 C r^{3 +} + 6 F e^{3 +} + 7 H_{2} O$
During the reaction, the oxidation number of $C r$ decreases from +6 to +3. Net decrease in the oxidation number of one $C r$ atom is $6 - 3 = 3$ . For 2 $C r$ atoms (in dichromate ion), the total decrease in the oxidation number is $2 \times 3 = 6$
The gram equivalent weight $= \frac{gram molecular weight}{Total change in the oxidation number} = \frac{294}{6} = 49$

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Similar questions

294 g

C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 C r^{3 +} + 7 H_{2} O

K_{2} C r_{2} O_{7}

= M

B r O_{3}^{-}

B r^{-}

B r_{2}

K B r O_{3}

x S n^{2 +} + y C r_{2} O_{7}^{2 -} + z H^{+} \to a S n^{4 +} + b C r^{3 +} + c H_{2} O

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