For reduction of dichromate, balanced reaction is : $Cr_2 O_7^{-2}(aq)+6 e^{-}+14 H^{+}(aq) \rightarrow 2 Cr^{3+}(aq)+7 H_2 O(l)$ $\qquad 3 mol \qqu

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For reduction of dichromate, balanced reaction is : $Cr_2 O_7^{-2}(aq)+6 e^{-}+14 H^{+}(aq) \rightarrow 2 Cr^{3+}(aq)+7 H_2 O(l)$ $\qquad 3 mol \qquad 1 mol$ $\text { Number of Farads required }=3 mol$ $\text { Let current }=I \text { amperes }$ $\Rightarrow \frac{I \times 48.25 \times 60}{96500}=3$ $I=100 A$

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In an electrochemicalcell, dichromate ions in aqueous acidic medium are reduced to $Cr ^{3+}$. The current $($in amperes$)$ that flows through the cell for $48.25$ minutes to produce $1$ mole of $Cr ^{3+}$ is $....$ . Use: $1$ Faraday $=96500 C mol ^{-1}$

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In an electrochemicalcell, dichromate ions in aqueous acidic medium are reduced to $Cr ^{3+}$. The current $($in amperes$)$ that flows through the cell for $48.25$ minutes to produce $1$ mole of $Cr ^{3+}$ is $....$ . Use: $1$ Faraday $=96500 C mol ^{-1}$

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