We have to determine what mass of magnesium is formed by electrolysis when a current of 9.5×104 A for a period of 26 hours.
We will follow these steps to solve this problem:
Step 1: Write an equation for the reduction of MgCl2 to Mg metal.
Step 2: Determine the current passed through the cells at 96 % efficiency.
Step 3: Determine the amount of electric charge passed through the cells.
Step 4: Calculate the amount of Mg metal formed.
Magnesium is obtained by electrolysis of molten MgCl2.
Several cells are connected in parallel by very large copper buses that convey current to the cells. Assuming that the cells are 96 % efficient in producing the desired products in electrolysis, what mass of Mg is formed by passing a current of 9.5×104 A for a period of 26 hr?
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Electrolysis of Water & Mixture of Ions concept. If you need more Electrolysis of Water & Mixture of Ions practice, you can also practice Electrolysis of Water & Mixture of Ions practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Kulatunga's class at USF.