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Electrochemistry question

2016 · Q90
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Electrochemistry question

2016 · Q90

NEETChemistryElectrochemistryMCQ+4 / −1
During the electrolysis of molten sodium chloride, the time required to produce 0.10 mol of chlorine gas using a current of 3 amperes is
  1. A
    55 minutes
  2. B
    110 minutes
  3. C
    220 minutes
  4. D
    330 minutes
View written solutionFree

Correct answer: B

At cathode : 2Na+

  • 2e– →\to→ 2Na

    At anode : 2Cl– →\to→ Cl2
  • 2e–
    ----------------------------------------------

    Net reaction: 2Na+
  • 2Cl– →\to→ 2Na + Cl2

    From Faraday’s first law of electrolysis,

    w = Z×\times×I×\times×t

    = {E \over {96500}}$$ \times I×\times×t

    No. of moles of Cl2 gas × Mol. wt. of Cl2 gas

    = Eq. wt. of Cl2 gas×I×t96500{{Eq.\,wt.\,of\,C{l_2}\,gas \times I \times t} \over {96500}}96500Eq.wt.ofCl2​gas×I×t​

    ⇒\Rightarrow⇒ 0.10 ×\times× 71 = 35.5×3×t96500{{35.5 \times 3 \times t} \over {96500}}9650035.5×3×t​

    ⇒\Rightarrow⇒ t = 0.10×71×9650035.5×3{{0.10 \times 71 \times 96500} \over {35.5 \times 3}}35.5×30.10×71×96500​

    = 6433.33 sec

    = 107.22 min ≃\simeq≃ 110 min
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