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The Recovery of Copper in Sulphide Ores by Roasting, Leaching, and Electrolysis Jack S

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The Recovery of Copper in Sulphide Ores by Roasting, Leaching, and Electrolysis Jack S Montana Tech Library Digital Commons @ Montana Tech Bachelors Theses and Reports, 1928 - 1970 Student Scholarship 6-3-1932 The Recovery of Copper in Sulphide Ores by Roasting, Leaching, and Electrolysis Jack S. Greenough Follow this and additional works at: http://digitalcommons.mtech.edu/bach_theses Part of the Environmental Engineering Commons, Geology Commons, Metallurgy Commons, Other Engineering Commons, and the Other Materials Science and Engineering Commons Recommended Citation Greenough, Jack S., "The Recovery of Copper in Sulphide Ores by Roasting, Leaching, and Electrolysis" (1932). Bachelors Theses and Reports, 1928 - 1970. 21. http://digitalcommons.mtech.edu/bach_theses/21 This Bachelors Thesis is brought to you for free and open access by the Student Scholarship at Digital Commons @ Montana Tech. It has been accepted for inclusion in Bachelors Theses and Reports, 1928 - 1970 by an authorized administrator of Digital Commons @ Montana Tech. For more information, please contact [email protected]. TEE RECOVERY OF COPPER IN SULPHIDE ORmS jjY ROASTING, LEACHING, AND ELECTROLYSIS. :sy SACK S. GREENOUGH. BUTTE. .MON1'ANA,. .J'U'.NE 3. I932. ~.'. ' .. ':" .... ;..~ .... , THE RECOVERY OF COPPER IN SULPHIDE ORES BY ROASTING, LEACHING, AND ELECTROLYSIS. Inaugural Thesis submitted as a partial fullfillment of the requirements for the degree of Bachelor of Science in Metallurgical Engineering from the Montana School of Mines. by Jack S. GTeenough Bu-cte, Monta-na.. toPY 2-' MONTANA SCij.OOL OF MiNES LiBRARY: BUTTE 42876 Butte, Montana, TABLE OF CONTENTS. PAGE. Theoretical Considerations ••••••••••••••••••••••• I Roast ing •......................................• :3 Results of Roasting, Table I, • •• •• •••• •• ••• •••• • 4 Curves: Fig. I, The Formation of Copper Sulphate with Time ••• 6 Fig. 2, Decomposition of Copper Sulphide with Time ••• 7 ~ig. 3, Formation of·Copper Oxide with Time •••••••••• 8 Fig. 4, Change in Total Copper with-Time •••••••••••• 9 Fig. 5, Formation of Soluble Iron with Time ••••••••• IO Leaching Tests •• w •••••• , •••••• , •••• ~ •••••••••••••••• II Results of Leaching Tests, Table II, ••••••••••••••• 12 Curves: - Figures 6a to 9b, ••••••••••.•••••••••••••• 13 to 16 Electrolysis of the teach Solution ••~ •••••••••••••• 17 Diagram Showing Electrical Connections ••••••••••••• 18 Results-of Electrolysis, Table III, •••••••••••••••• 20 Conclusions •••• ~•••••••••••••••••••••••••••••••••.• 21 I. THEORETICAL CONSIDERATIONS. Sulphide ores of copper are insoluble in dilute sulphuric acid leaching solutions, but a very high extraction ean be obtained if the copper ore is in the oxidized condition. The problem is to convert the sulphide~lntQ~the oxide form. This can be done by giving the sulphide ore an oxidiz~ng-sulphatizing roa.st; Copper sulphate is soluble in water, so acid will be saTed in the leaching process if copper sulphate is present. The iron in the copper sulphide ores is present as pyrite, or in combinations as bornite, or chalcopyrite. The object of the roast is to convert a,considerable portion of the copper to the oxide form and a lesser amount to the form of sulphate; and all of the iron to ferric oxide,Fe203• which is insoluble in dilute acid. If iron existed in the electro- lyte, the current efficiency would be lowered to a considerable degree, since the iron is oxidized to the ferric condition at the anode and is reduced ·to ferrous iron at the cathode, thus consuming current which· might otherwise be used to deposit copper. The decomposition temperature of copper sulphate i8 650 degrees Centigrade and that of ferrous sulphate is 590 degrees centigrade,(I)Bo that theoretically the correct temp- erature of roasting should exist between 600 and 650 degrees Centigrade. (I) "Hydrometallurgy Of Copper", by William E.Greenawalt. 2. By roasting at this temperature, a maximum amount of copp~r oxide and of copper sulphate and a minimum amount of soluble iron should be obtained. After the ore has been r0asted and leached, the result- ing solution is transferred to the electrolytic tanks, where it is electrolyzed using insoluble anodes. The anode used was lead while the cathode was copper. For every pound of cop~er deposited at the cathode, 1.54 pounds of sulphuric acid will be regener- ated. The ideal working plan is to regenerate enough acid at the anode SO that it will not be necessary to buy any for leach- ing purposes. If there are preoious metals present, they will occur in the residue. According to Greenawalt, they can be recovered by cyanidation, chloridizing, or by direct smelting. He states(2) that the cyaniding of material which has alreadY been finely ground and leached to remove cyanicides i8 a cheap and simple _\ process and the preoious me~alsare produced in bullion form, acoeptable to the U.S. Mint. Experimental work indicates that with properly roasted concentrate there will be no difficulty in cyaniding the copper leached residue at a cost of $0.50 to $1.00 per ton. (2) American Electro-Chemical Society, Pre-print 61-29, "Electrometallurgy Applied to COPJ?er and to Complex Ores". By, W.E.Greenawalt. ROASTING. The material used in the present investiga~ion was Anaconda copper flotation concentrate, containing 26.42 % eu and 22.95 % Fe, the size varying from 100 to 2240 mesh. Two hundred grams were weighed out, placed in a large roasting dish and roasted in an electric muf~le, with a plentiful supply of air and with frequent rabbling; the temperature was 600 degrees Centigrade. A sample was taken from the main roast at half hour intervals and analyzed for water soluble copper, acid soluble copper (1:9 RCI), insoluble copper, and soluble iron. In analyzing the samples, the copper existing as sul- phate was found by boiling in 100 cc., of water for three minutes, filtering, and titrating with potassium cyanide until the blue color formed by the addition of ammonium hydroxide dissappeared. The oxide copper was found by leaching the above residue with 100 cc., of boiling 1:9 RCI for three minutes, filtering and titrating as indicated in the preceding determination. The cop- per as sulphide was determined by dissolving the residue from the last step in hydrochloric acid and stannous chloride and titrating with potassium cyanide. The iron was determined by precipitating it with ammonium hydroxide, and analyzing it by the permanganate method. Total coppers were also run and these results cnecked very closely with the values obtained by adding the oxide, sulphate, and sulphide forms of copper. MONTANA SCHOOL OF MIN ss LI.... ARY BUTTE 4. TABLE I. Roasting Copper as . Copper as Copper as Soluble Time,hrs. Sulphate,%. Oxide,%. Sulphide,%. Iron,%. t 0.00 41.6 58.4 6.60 I 0.00 51.5 48.5 23.'70 It 10.00 78.1 11.9 22.50 ... 2 20.10 79.0 0.9 4.90 2t 31.00 69.0 0.0 I.65 3 25.80 74.20 0.0 I.50 3t 30.00 70.00 0.0 1.50 4 32.70 67.30 0.0 1.60 5. The results-are shown in Table I. These results were also plotted and will be seen by observing Figures I,2,3,4,and5. Figure I illustrates the formation of copper sulphate with the time of roasting. It is seen that no copper sulphate was formed· until the material had been roasted for one hour. The percentage of the total copper in the form of sulphate steadily increased until after two and one-half hours of roasting, when it reached 30 per-ccerrt, - Figure 2 correlates the decomposition of copper sulphide with the time of roasting. When the first sample was taken for analysis at the end of a.roasting period of half an hour it is observed that 58 per-cent of the total copper existed in the form of sulphide,but as the roasting progressed this value steadily decreased until at the end of two and one- half hours it became zero. The formation of copper oxide with roasting time is illustrated in Figure 3. At the end of two and one-half hours of roasting, 70 per-cent of the total copper·was in the oxide form. As roasting progresses the volatile constit- uents were expelled so that the percentage of total copper increased. This is shown by Figure 4. The behavior of acid-soluble iron in this type of roast is shown in Figure 5. No water soluble iron was form- ed. The percentage of a~id-'Boluble iron increased from 0 to 23.90 per-cent in a roasting period of one hour and then decreased until it became I.6 .per-cent at the end of two and 6. Figure I. , 23 -i' ·F I-t-t-I-H 21 +t+t+t+rt, ., I 19 I, 18 , , 17 16 ., 6 _ 27: (110 U~S). Figure 2~ 24 I---H-++-f-Hit - t ,-1 23 22 I I 21 n I I I 19 " I + :-1+ +r- -++ 18 I I H-++-JI I I 11 C-'. -+~+J:- -I 17 I I I I " I 16 I t- I, 15 i -:V I I -+- +- 14 1"- - 13 I I - _ _I _E +H---H-H H-H-H -I t, 12 ~ 11 10 T 9 8 I, • 7 6 I I 1\- ,- o . 3 8. Figure 3. 24 _"T + ! + Ii H:: I I f- H- + 23 I! i : I T -1 ~t + T" I Ii-.' -~I- ' 22 -~t-- ;- 1 - 1 I I -I 21 in ' - 1-1- I - 1- ~- I -f~- I-J ~, -I- -- -1 -~ ru, 19 - ,,~ I I~ I f - t . ~t!f-~ -+ I , F - =i-I - " 18 -!. +- --II-, -+ l -'-i -F f-I • 1 - - I 17 r::-I 16 -~ 15 I P. -~ p~ :t 14 -~ Itt..,- ! -1- I - - 13 - ~I ! I 'j -1 - --- -- - --- - 12 --- ---- 11 ~, 10 9 8 =N. 7 '+ I 6 '-1 I tr + _j- 5 ,+ J I , -- , I - ..... 1 Q I tFI -+- I- 1- fi- 311 -F - -- +- 2 ++: i-, f/ 1 IT + ..
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