Effect of Manganese and Arsenic upon Current Efficiency in the Deposition of Zinc from Zinc Sulphate Solution

Throughout the entire experiment the electrolysis were conducted in an eight-hundred cubic centimeter beaker. An excellent circulation of the solution was assured by means of an electric stirrer, vigorous gas evolution from the anodes, and by means of a regulated feed-discharge system. By means of this balance, solution of the same impurity concentration as that of the electrolyte was fed in the cell just as fast as the discharge was syphoned out.

Copper Commando Index – vol. 1

Index for volume 1 (Aug. 1942-Aug. 1945) lists personal names, places, subjects; page and issue numbers.

Copper Commando Index – vol. 2

Index for volume 2 (Aug. 1942-Aug. 1945) lists personal names, places, subjects; page and issue numbers.

The Effect of the Cu:Fe''' Ratio Upon the Current Efficiency in the Electrolysis of a Copper Sulfate Solution Containing Iron Sulfate

It is a well-known fact that, in the electrolysis of a CuSO4 solution containing iron sulfate, using insoluble anodes, with the depletion of copper, the point is finally reached where the current efficiency becomes zero. This decrease in current efficiency is due to the oxidation of the ferrous sulfate to the ferric condition at the anode, by the oxygen liberated. The resulting ferric sulfate diffuses over to the cathode and there dissolves copper from the cathode according to the chemical equation Cu + Fe2 (SO4)3 = CuSO4 + 2FeSO4. This copper, which has been deposited at the cathode by the electric current, is thus redissolved by the Fe2(SO4)3. The solution of the copper causes at the same time a formation of FeSO4 which in turn diffuses over to the anode and is there oxidized to Fe2(SO4)3; and so the cycle continues, using electric current without rendering useful work. E. H. Larison has noted that a definite amount of ferric salts must be reduced to the ferrous condition before all the copper will remain on the cathode; he does not state, however, just what this point is. L. Addicks has plotted the relation between current efficiency and ferric sulphate content. The existence of the results scattered the points more or less, although the decrease in current efficiency with increased ferric sulphate content is clearly indicated. E. T.Kern has likewise noted that the smaller the amount of copper in the solution, the greater is the reduction of current efficiency. In this work, therefore, it was desired to determine what amount of ferric iron was permissible in a copper sulfate solution of definite concentration before the current efficiency would drop to zero, and what, if any, was the effect of definite Cu:Fe’’’ratio upon the current efficiency of the electrolysis.

Copper Commando Index - volumes 1, 2, and 3

Index for volumes 1, 2, and 3 (Aug. 1942 - Aug. 1945) lists personal names, places, subjects; page and issue numbers.

The Rate of Precipitation of Copper Aluminide in the Silver Rich Silver-Copper-Aluminum Alloys

In order to determine the best annealing temperature at which to age-harden the alloys, hardness tests on speci­men annealed for different lengths of time at different temperatures were made.

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

Sulphide ores of copper are insoluble in dilute sulphuric acid leaching solutions, but a very high extraction can be obtained if the copper ore is in the oxidized condition. The problem is to convert the sulphide into the oxide form. This can be done by giving the sulphide ore an oxidizing-sulphatizing roast. Copper sulphate is soluble in water, so acid will be saved 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 Effect of the Fe2: Fe3 Ratio upon the Current Efficiency in the Electrolysis of a Copper Sulfate Solution Containing Iron Sulfate

In the treatment of copper ores by hydro-electro-metallurgical methods, not only is copper deposited, but other metals are also dissolved. In practice it has been found* that iron, under certain conditions, causes the copper to deposit on the cathode as a nonadherent precipitate and also that the iron in solution causes a great decrease in current efficiency, es­pecially when the electrolysis is conducted by operating with a higher current density at the cathode than at the anode. The present investigation deals with the effects of the two valences of iron on the current efficiency and endeavors to determine whether or not there is a ratio of the two at which point the efficiency becomes zero or approaches it.

Some Notes on the Composition of "Copper Pitch"

A supply of so-called "copper pitch" ore was received by the Montana Bureau of Mines and Geology in response to a request by them from a resident of Kalispell, who had previously sent a specimen to the Bureau for a mineralogical analysis. Since this material was little known and had apparently received but little study under a reflec­ting microscope, it was thought that such a study might throw some light on the mineralogical and chemical composition of the material.

Leaching Copper Minerals in the Butte District

The history of mining in Butte is woven about three of our principal metals. The gold placers first attracted the attention of miners in 1863, and reached their peak production in 1867. Silver was the second metal mined, and this operation required the erection of large mills with a consequent increase in mining activity that made the district a prominent producer. Although the presence of copper in the silver ore had been known, the credit for the first development of the copper veins is due Senator W. A. Clark. The original Colusa, Mining Chief, and Gambetta claims were developed to 1872. The ore was freighted by wagon trains 400 miles to Corrine, Utah, thence by rail eastward, some of it going to Swansea, Wales. The cooper production of the "richest hill on earth" has mounted to ten billion pounds.

The Equilibrium Relations of Nickel Sulfide with Copper and Sodium Sulfides

The equilibrium relations of many of the metallic sulfides have long been a source of scientific and commer­cial interest, of particular interest, are the sulfides of nickel and copper, since the economic recovery of both of these useful metals, from their ores, involves the formation of a sulfide at some stage of the operations.

Precipitation of Gold, Silver, and Copper from Cyanide Solutions on Activated Charcoal.

Charcoal has been known for a considerable length of time to have the property of recovering gold, silver, and copper from cyanide solutions of these metals. Quantita­tive data that may shed light on the mechanism of the re­moval of these metals is very limited except that char­coal in a form known as activated has the power to abstract gold and silver in considerable quantities from the above solutions.

Roasting and Leaching Bulk Copper-Zinc Sulfide Concentrates with the Subsequent Recovery of the Metals by Electrolysis

The aim of this research was to investigate the possibilities of roasting and leaching a bulk copper-zinc sulfide concentrate, and the subsequent separation of the metals from the leach solution by electro­lytic deposition.

Electrolytic Recovery of Copper and Zinc from Brasses

Reclaimed metals, or secondary metals, are becoming of great im­portance in the metal industries of the world. Secondary metals are an important factor in production. The increase in the secondary production of copper is due to many factors. One of these may be its permenance, that is, the metal does not corrode very readily. Another reason for increase in production is the high price paid for it.

A Preliminary Study of Montana Copper - Nickel Ore

Deposits of sulfides, containing nickel and copper with associated platineferous minerals occur in the Stillwater Igneous Complex. This is a group of unusual igneous rocks situated in Stillwater and Sweetgrass counties in Montana.