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Electrolysis of molten MgCl2 is the final production step in the isolation of magnesium from seawater by the Dow process. Assuming that 38.0 g of Mg metal forms, answer the following questions. (a) How many moles of electrons are required? 2 mol e− (b) How many coulombs are required? 1.93 × 10 5 C Enter your answer in scientific notation. (c) How many amps will produce this amount in 3.50 h? A

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Answer:

24.25A

Explanation:

Mg(aq) + 2e --------> Mg(s)

Two moles of electrons are required

1 mole of electron requires 1F of electricity

1F= 96500C

Since 2 moles of electrons are involved, 2F are involved that means 2×96500= 1.93×10^5C.

Mass of Mg produced from reduction equation=24g

But q=It and t must be in seconds.

If 1.93×10^5C produces 24g of Mg

3.5×60×60×I will produce 38.0g of Mg

Therefore I= 24.25A

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