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

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

20 drops hope this

here is table 2-2:

country

percent of eligible voters that voted

rank

united states

44.9%

138

canada

60.1%

107

costa rica

84.6%

14

hungary

66.9%

82

japan

57.0%

118

egypt

27.7%

159

south africa

85.5%

10

ans is no, the data set cannot be plotted as a single circle graph