Final answer:
The production of sodium metal through electrolysis and requires the use of Faraday's laws to calculate the mass produced. The correct answer is d) 100 kg, under the assumption of a 100% yield from the process.
Step-by-step explanation:
The electrochemical production of sodium metal using a process known as electrolysis. Specifically, it's asking for the amount of sodium produced from a given current, assuming a 100% yield. This is a typical question in the field of electrochemistry, where Faraday's laws of electrolysis can be applied to predict the production of substances during electrolysis.
To solve such a problem, one would employ Faraday's first law of electrolysis, which states that the amount of a substance deposited or liberated at an electrode is directly proportional to the charge (or, equivalently, the product of current and time). However, since the problem only presents an assumed yield rather than requiring the calculation of mass, we can conclude that for a 100% yield, the production would be equal to the 100 kg as initially stated, being option d) 100 kg.
Remember that for a real-life scenario, yields are rarely 100% due to inefficiencies and side reactions, but for the sake of this exercise, the assumption simplifies calculations.