An acidic solution of dichromate is electrolyzed for 8 minutes using 2A current. As per the following equation
Cr₂O₇^2- + 14H⁺ + 6e^– $\to$ 2Cr³⁺ + 7H₂O
The amount of Cr³⁺ obtained was 0.104 g. The efficiency of the process(in%) is (Take : F = 96000 C, At. mass of chromium = 52) ______.

Cr₂O₇^2- + 14H⁺ + 6e^– $\to$ 2Cr³⁺ + 7H₂O <br><br>I = 2 A, t = 8 min <br><br>From 1^st law of faraday, <br><br>w_Cr⁺³ = z $\times$ i $\times$ t <br><br>$\Rightarrow$ w_Cr⁺³ = ${{52} \over {96000 \times 3}} \times 2 \times 8 \times 60$ <br><br>= ${{52} \over {300}}$ <br><br>Mass of Cr³⁺ ions actually obtained = 0.104 gm <br><br>% efficiency = <span style="display: inline-block;vertical-align: middle;"> <div style="text-align: center;border-bottom: 1px solid black;">Actual obtained Amt</div> <div style="text-align: center;">Theo. obtained Amt</div> </span> $\times$ 100 <br><br>= ${{0.104} \over {{{52} \over {300}}}}$ $\times$ 100 <br><br>= 60 %