Anthracene, C14H10, can be oxidized to anthraquinone, C14H8O2. What weight of anthraquinone can be produced by the passage of a current of 1 A of 40 min if the current efficiency is 96.5%?

Question

Prashant Kotian · Accepted Answer

Correct answer: B. Oxidation reaction: C14H10 + 2H2O -> C14H8O2 + 6H^+ + 6e^– (n-factor = 6). Total charge passed = 1 A × (40 × 60) s × 0.965 (efficiency) = 2316 C. Faradays passed = 2316 / 96500 = 0.024 F. Moles of anthraquinone produced = 0.024 / 6 = 0.004 mol. Molar mass of C14H8O2 = 168 + 8 + 32 = 208 g/mol. Mass = 0.004 × 208 = 0.832 g. Therefore, correct answer is B.

💡 Solution & Explanation

Practice 22,000+ questions like this