Consider the reaction:
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O
What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr₂O₇²⁻?
Approved Tutor Answer11 Months agoTo determine the quantity of electricity required to reduce 1 mole of Cr₂O₇²⁻, we can use Faraday's law of electrolysis. The reaction shows that 6 moles of electrons (e⁻) are needed to reduce 1 mole of Cr₂O₇²⁻.
The charge (Q) in coulombs can be calculated using the formula:
Q = n × F
where:
Now, substituting the values:
Q = 6 moles × 96485 C/mol = 578910 C
Thus, the quantity of electricity needed to reduce 1 mole of Cr₂O₇²⁻ is approximately 5.79 × 10⁵ C. Therefore, the correct answer is:
B. 5.79 × 10⁵ C
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