Electrolysis of molten MgCl 2 is the finalproduction step in the isolation of ma

Question

Electrolysis of molten MgCl2 is the finalproduction step in the isolation of magnesium from seawater.Assuming that 37.8 g Mg metal forms, calculate the following. (a) How many moles of electrons are required? (b) How many coulombs are required?
(c) How many amps are required to produce this amount in 1.75h? Electrolysis of molten MgCl2 is the finalproduction step in the isolation of magnesium from seawater.Assuming that 37.8 g Mg metal forms, calculate the following. (a) How many moles of electrons are required? (b) How many coulombs are required?
(c) How many amps are required to produce this amount in 1.75h?

Explanation / Answer

Mg2+ + 2e- => Mg a) 37.8 grams mg *(1mol Mg/24.31 grams)*(2mol e-/1mol Mg) = 3.11moles ep b) 1 mol e- = 96485 C 3.11 moles e- *(96485 C/1mol) = 3.00 e5 C c) 1 A = 1 C/s (3.00e5 C)/(1.75 hr *60 min/hr *60sec/hr) = 47.62 Amps

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