(a) Magnesium is obtained from seawater. If the concentration of Mg 2+ in seawater is 0.050 M,...
Question:
(a) Magnesium is obtained from seawater. If the concentration of Mg2+ in seawater is 0.050 M, what volume of seawater (in liters) must be treated to obtain 1.00 kg of magnesium metal? What mass of lime (CaO; in kilograms) must be used to precipitate the magnesium in this volume of seawater?
(b) When 1.2 × 103 kg of molten MgCl2 is electrolyzed to produce magnesium, what mass (in kilograms) of metal is produced at the cathode? What is produced at the anode? What is the mass of this product? What is the total number of Faradays of electricity used in the process?
(c) One industrial process has an energy consumption of 18.5 kWh/kg of Mg. How many joules are required per mole (1 kWh = 1 kilowatt-hour = 3.6 × 106 J)? How does this energy compare with the energy of the following process?
MgCl2(s) → Mg(s) + Cl2(g)
Step by Step Answer:
Chemistry And Chemical Reactivity
ISBN: 9780357001172
10th Edition
Authors: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel