How much current is necessary to produce H2 gas at the rate of 1 cm3 per second under STP?
Correct answer: C. 8.61 amp
- A. 4.305 amp
- B. 17.22 amp
- C. 8.61 amp
- D. 2.1525 amp
Explanation
The correct answer is 8.61 amp. To determine this, we utilize Faraday's laws of electrolysis, which state that the amount of substance liberated at an electrode is directly proportional to the quantity of electricity passed. At STP, 1 mole of hydrogen gas occupies 22.4 liters, and thus 1 cm3 corresponds to 4.464 x 10-5 moles of H2. Using Faraday's constant (approximately 96485 C/mol) and the fact that 2 moles of electrons are needed to produce 1 mole of H2, the required current is calculated to be 8.61 amp. The other options result from either incorrect application of these principles or computational errors.
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