An acidic solution of dichromate is electrolyzed for 8 minutes using 2 A current. As per the following equation
${Cr}_{2} O_{7}^{2} + 14 H^{+} + 6 e^{-} \to 2 {Cr}^{3 +} + 7 H_{2} O$
The amount of ${Cr}^{3 +}$ . obtained was $0.104 g$ . The efficiency of the process $(in %)$ is (Take : $F = 960000 C$ , At. mass of chromium $= 52$ )

Question

An acidic solution of dichromate is electrolyzed for 8 minutes using 2 A current. As per the following equation

${Cr}_{2} O_{7}^{2} + 14 H^{+} + 6 e^{-} \to 2 {Cr}^{3 +} + 7 H_{2} O$
The amount of ${Cr}^{3 +}$ . obtained was $0.104 g$ . The efficiency of the process $(in %)$ is (Take : $F = 960000 C$ , At. mass of chromium $= 52$ )

Aicharya · Accepted Answer

Charge q = it = 2 &#215; 8 &#215; 60 = 960 &#160; C 960 96000 = 0 . 01 F Cr 2 O 7 2 - + 14 H + + 6 e - &#160; &#8594; &#160; &#160; 2 Cr 3 + &#160; + &#160; 7 H 2 O 0 . 01 F &#160; &#160; &#160; 1 3 &#215; 0 . 01 &#160; mole Theoritical mass of Cr 3 + = 1 3 &#215; 600 96000 &#215; 52 = 0 . 173 g So, efficiency = W actual W Theoritial &#215; 100 = 0 . 104 0 . 173 &#215; 100 = 60 %

An acidic solution of dichromate is electrolyzed for 8 minutes using 2 A current. As per the following…

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