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An electrolysis cell consumed a charge of 4.00 C in 5.00 minutes - VCE - SSCE Chemistry - Question 9 - 2021 - Paper 1

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An electrolysis cell consumed a charge of 4.00 C in 5.00 minutes. This represents a consumption of A. 4.15 x 10^-3 mol of electrons. B. 2.07 x 10^-4 mol of electrons... show full transcript

Worked Solution & Example Answer:An electrolysis cell consumed a charge of 4.00 C in 5.00 minutes - VCE - SSCE Chemistry - Question 9 - 2021 - Paper 1

Step 1

Calculate the number of moles of electrons consumed

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Answer

To find the number of moles of electrons consumed, we use the formula:

n=QFn = \frac{Q}{F}

where:

  • nn = number of moles of electrons
  • QQ = charge in coulombs
  • FF = Faraday's constant (approximately 96485 C\/mol96485 \, C \/ mol)

Substituting the known values:

n=4.00 C96485 C\/mol≈4.15×10−5 moln = \frac{4.00 \, C}{96485 \, C \/ mol} \approx 4.15 \times 10^{-5} \, mol

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