Part A. How many kilowatt-hours of electricity are used to produce 4.00 kg of ma

Question

Part A. How many kilowatt-hours of electricity are used to produce 4.00 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 5.00 V?

Part B. What is the reducing agent in the redox reaction represented by the following cell notation?
Mn(s) | Mn 2+(aq) || Ag+(aq) | Ag(s)

Part C. Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Cr(OH)4- and ClO- in the balanced reaction?
Cr(OH)4-(aq) + ClO-(aq) CrO42-(aq) + Cl-(aq)

Explanation / Answer

average atomic weight of magnesium is 24.3 g/mol.

Moles of magnesium = 4.00 kg/(24.3 g/mol) = 164.6 mol

Reaction is Mg ------> Mg2+ + 2e-

Power, P = 164.6 mol*(2 F/mol Mg)*(96500 C/F)*5.0 V*(1 kWt/3.6*106 J)

= 44.1 kWt

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