An acidic solution of dichromate is electrolyzed for 8 minutes using 2 A current. As per the following equation Cr_2O72+14H^(+)+6e^(-)→2Cr^(3+)+7H_2O…

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 $= 52$ )

MARKS Content Team · Accepted Answer

Correct answer: 60. Charge q=it=2×8×60=960 C 960/96000=0.01F Cr_2O72-+14H^(+)+6e^(-) → 2Cr^(3+) + 7H_2O 0.01F 1/3×0.01 mole Theoritical mass of Cr^(3+)=1/3×600/96000×52=0.173g So, efficiency =W_actualW_Theoritial×100=0.104/0.173×100=60%

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An acidic solution of dichromate is electrolyzed for 8 minutes using 2 A current. As per the following equationCr2O72+14H++6e-→2Cr3++7H2OThe amount of Cr3+. obtained was 0.104g. The efficiency of the process (in%) is (Take : F=960000C, At. mass of chromium =52)

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