This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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a) The formula of the major ore of copper metal is chalcopyrite. CuFeS_2 b) Process (II) is froth flotation. c) The reaction that occurs in stage (III) is the roasting of chalcopyrite in air to produce copper(I) sulfide and iron(II) oxide. 2CuFeS_2(s) + 4O_2(g) → Cu_2S(s) + 2FeO(s) + 3SO_2(g) d) In stage (IV), copper(I) sulfide is heated in a converter with air and sand (SiO_2). Iron impurities are oxidized to FeO, which reacts with SiO_2 to form FeSiO_3 slag. The Cu_2S then undergoes self-reduction: some is oxidized to Cu_2O, which reacts with remaining Cu_2S to produce molten copper and SO_2 gas. This molten copper is blister copper. e) The half-cell equations for the reactions occurring at the anode and cathode in stage (VII) (electrolytic refining) are: At the anode (oxidation): Cu(s) → Cu^2+(aq) + 2e^- At the cathode (reduction): Cu^2+(aq) + 2e^- → Cu(s)