The lead storage battery as it is used today is made up of the pasted type plates of lead dioxide, the anode, and sponge lead, the cathode, and wooden or hard rubber separators, which serve to insulate these from one another. In manufacturing these, it is desirable to keep them free from impurities

McCracken, George A.

Digital Commons @ Montana Tech

Montana Tech LibraryDigital Commons @ Montana TechBachelors Theses and Reports, 1928 - 1970 Student Scholarship1-1-1935The Effects of Zinc Sulphate, Manganese Sulphate,and Iron Sulphate on the Lead Storage Cell.George A. McCrackenFollow this and additional works at: http://digitalcommons.mtech.edu/bach_thesesPart of the Ceramic Materials Commons, Environmental Engineering Commons, GeologyCommons, Geophysics and Seismology Commons, Metallurgy Commons, Other EngineeringCommons, and the Other Materials Science and Engineering CommonsThis Bachelors Thesis is brought to you for free and open access by the Student Scholarship at Digital Commons @ Montana Tech. It has been acceptedfor inclusion in Bachelors Theses and Reports, 1928 - 1970 by an authorized administrator of Digital Commons @ Montana Tech. For moreinformation, please contact astclair@mtech.edu.Recommended CitationMcCracken, George A., "The Effects of Zinc Sulphate, Manganese Sulphate, and Iron Sulphate on the Lead Storage Cell." (1935).Bachelors Theses and Reports, 1928 - 1970. Paper 58.McCracken, G.ATHE EFFECTS OF ZINC SULPHATE, MANGANESE SULPHATE,AND IRON SULPHATE ON THE LEAD STORAGE CELLbyGEORGE A. McCRACKEN I~.IA ThesisSubmitted to the Department of Chemistryin Partial l!'"1ulfillment-or theRequirements for the Degree ofBachelor of Science in Metallurgical EngineeringMONTANA SCHOOL OF MINESBUTTE, MONTANA1935THE EFFECTS OF ZINC SULPHATE, MANGANESE SULPHATE,AND IRON SULPHATE ON THE LEAD STORAGE CELLbyGEORGE A. McCRACKENSubmitted to th;h;:~:rtment Of,~~:~t'tin Partial Fulfillment of theRequirements for the Degree ofBachelor of Science in Metallurgical Engineering//Z31MONTANA SCHOOL OF MINESBUTTE, MONTANAMAY Z, 1935•TABLE OF CONTENTSPageIntroduction~ •••••••••••••••••• ,.~•••••lApparatus and Reagents ••••••••••••••••• lExperimental Procedure 5Results and Discussions •••••••••••~••••?Conclusions ••••••••••••••••••••••••••• llBibliography~ ••••••••••••••••••~••••••13-1-THE EFFECTS OF ZINC SULPHATE, MANGANESE SULPHATE,AND IRON SUL.PHATE ON THE LEAD STORAGE CELLThe lead storage battery as it is used today is madeup of the pasted type plates of lead dioxide, the anode,and sponge lead, the cathode, and wooden or hard rubberseparators, which serve to insulate these from one another.In manufacturing these, it is desirable to keep them freefrom impurities. This is impossible for small amountswill get in with the water, acid or even from the steeltools which contact the cell during its construction orrepair. The most common impurities entering a cell in thismanner would be iron and manganese. It is evident that these,each with the possibility of having more than one valence,would be oxidized at the anode and reduced at the cathode.This results in sulphating both plates and producing a lossof capacity. Another impurity which might also get into acell is zinc; it is not exactly known how this would reacton a cell. In order to study the definite effects of theseimpurities on a battery, this investigation was made. Thevoltage characteristics on charge and discharge, the selfdischarge, and the capacity of the lead storage cell werestudied with reference to the effects of the presence of zinc,manganese and iron in the electrolyte.APPARATUS AND REAGENTSFor the investigation, it was necessary to use at leasttwo cells to study the effects of each impurity, so that the-2-results of one could be checked against the other. Sevencell, in all, were used, each one being composed of twonegative plates, one positive plate, and inserted betweenthese were cedar separators. The plates used were manufacturedby The Henderson Battery Company of Spokane, Washington.The exact compositi0n of the materials used to prepare theseis not known, but "Arendt~ (Bibliography 1) says that, ingeneral, one part of litharge (PbO) and one part of 1.10to 1.15 specific gravity, sulphuric acid, whereas, that ofthe cathode is made up of five parts of litharge (PbO) andone part of 1.10 to 1.15 specific gravity, sulphuric acid.They also contain some filler, such as magnesium or bariumsulphate, or wood flour, to increase the porosity, for thisis an essential of a good plate since it allows acid to pene-trate the plates easily, thereby exposing a maximum of sur-face to the electrolyte. The plates, after being thoro~ghlydried, are placed in weak sulphuric acid (specific gravity1.15) and formed into a positive plate of lead dioxide (PbOZ>and a negative of sponge lead. The negative plates, as usedin this work, were thoroughly formed but the positive requiredabout ten or twelve hours to insure complete conversion toThe electrolyte was a solution of chemically puresulphuric acid and distilled water mixed in the properproportions to give a specific gravity of 1.275. The levelof the solution in the cell was maintained above the top ofthe plates to prevent exposure to the air for sponge lead-3-is very susceptible to oxidation and will take up carbondioxide; this has a tendency to harden and thus reduce thecapacity of the plate by clogging up its pores. The rapiditywith which this oxidation takes place was observed in onecase during this work when a set of plates upon removal ofthe electrolyte immediately developed a large amount of heatat their surfaces.Enough material was available to prepare seven of thesecells, which were placed in an old (12-volt} battery box,since this contained compartments that were of the size de-sired. Tests were made to be sure there were no breaks inthe partitions between cells.A copper coulometer, used to determine the capacitiesof the cells, was composed of three electrodes, two of whichwere anodes, and a solution of 150 grams of copper sulphateand 50 grams of alcohol per liter of water. The set-up isshown in Figure 2.For ordinary voltage readings a common Weston volt-meter functioned well, but for measuring potentials of areference electrode against each plate it could not beused, due to the fact that it contains only a low resist-ance and this allows current to flow through, thus introducingan error. Therefore, a potentiometer was more suitable.All the current readings were ascertained with a commonWeston ammeter.-4-The reference electrode (Bibliography 2) Was a stickof cadmium, three-eighths of an inch in diameter, immersedin a solution of sulphuric acid of a specific gravity of1.275. These were contained in a bottle that was sealed bya rubber stopper. The cadmium stick, and a long glass tub-ing, that was shaped in such a way that it could be immersedin the electrolyte of the battery cells, projected from thebottle and through the stopper. The glass tubing served tojoin the electrolyte of the half cell with that of thebattery cells. In all cases, the end of this connectiontube was placed against the plate in order to have the sameposition for each reading. This procedure is necessarybecause a reading taken with the tube placed away from theplate is different from that where it is set against theplate. Potentials of both plates were always positive tothe cadmium cell. The potential of the lead dioxide, asmeasured against this half cell, decreases on dischargebut it is at all times higher than that of the cell, andthe sponge lead potential will rise from 0.1 to about 0.3volts on completion of the discharge. The difference be-tween the cadmium-sponge lead and the cadmium-lead dioxidepotential at any moment equals the cell voltage for thecorresponding instant. All readings of Electromotiveforcewere taken on open circuit. The advantages gained in em-ploying the half cell as described here are the insolubilityof cadmium in sulphuric acid, thus insuring against any10 k ~'d cii e!Xl.,~ ~ IIG> ., ., 0,....., H a~ 1=1co 0 \-4 co..-l +> tlO iri ,....., 1=1 +>+>1Il1=l+> II G eo t>. ~ ~0)1=I!=l..-ls:l ~ V 1=1 ~ ..-lCI) ..-l 0) Q) ..-l!=l..-l() ,....., 0) HI ~ + +>CO;::l+> +>CO~~sr-fcO Q) 0o eo 0 v.p~+> r-fc.!:i ~rQP.CO.,~ Q)100 CO..-lG>t.!, J.bO,.....,15+> +>..-lE;:rQkJo+ ~ 0101R,.....,~!=l ~ Q) • co..-l()+>CD A-tp:.jrQ '1 ,....., •~Vb'd I • ,....., ~I I>.j + ;::l Q);::l Pi ~ o eO)~,.....,+> 0 •CO"""'Q)CO ::;;!ICD co .cI ~-+ >< s~ t>.P, o t) ·~§:~+> ~ co I%l..-l ..-l ~~ a: ~I>cI T ~i+>~ co .s:Ico ~ CD +> 0 v~ro.cg ,....., 'd co !=l +>cO ..-l t>. I § ..-l+ I>cI~I c.> ~ ..-l ,.....,~ • ~- +> C> rO ~ co 0f CD~CO!=l I~ • II co 0 Q) to ~ j:Q co ~ coI------------~Q]T..-1-b +ai 14-----+_L..--I•j:Q•15:'------t IIIIII f~-~ )- -_- -~-- -- -~~E:l 8~~(.)~~~H0~&3Hq (\l~~~~0IHg5 ~+ s ~r;ij I(.) 8~fI5+ ><~~~+-5-contamination of the battery, and the absence of a differ-ence of potential that would exist if the acid of the batterycell and half cell were not practically of the same concen-tration. The set-up used to read these potentials isillustrated in Figure 1.The solutions of zinc sulphate, iron sulphate, andmanganese sulphate were made from chemically pure materials.The first two of these were somewhat deprived of their waterof hydration, thereby making it necessary to determine theconcentration of the solutions by a volumetric analysis;the zinc was titrated against a standard solution of potassiumferrocyanide and the iron against a standard solution ofpotassium permanganate. The manganese sulphate was onlyslightly effloresced so that it was only necessary to makethe solution up of a definite amount of water and the salt.EXPERIMENTAL PROCEDUREIn this work impurities were added to the cells indefinite concentrations and their effects on the voltageof the cell, when on charge and discharge; on the selfdischarge; and on the capacity, were noted •.At first it was necessary to make a study of thecharacteristics of an uncontaminated cell to determine therate of charge and discharge to be used, and also to ascertainthe capacity of the normal cell at this rate of discharge.-6-Keeping the results of this investigation in mind,the other work was carried out as follows. 8ix more cellswere put into service, five of which contained the impurityto be studied, the other being left as a normal cell. Withthis arrangement the effects of the iron sulphate, manganesesulphate, and zinc sulphate 'could be noted by comparison withthe uncontaminated cell.The effects of impurities were studied in the concen-trations as tabulated below:Impurity added as a Concentration in grams ofImpurity water solution of metal per liter of ElectrolyteZinc Zn 8°4 7H2O .07395Zinc tt .14790Zinc tt .29580Zinc '"~ .369'75Zinc ", 7.39500Iron Fe 8°4 7H2O .014Iron "' .028Manganese n 8°4 2H2O .020Manganese " .040The cells contaminated with these various concentrationsof impurities were put through a number of cycles of chargingand discharging at a constant current rate of two amperes.Before drawing the energy from the charged cell, it was leftidle for a period of ten or twelve days. The cells, when on-7-the charging line, were assumed to contain a maximum ofenergy when a voltage of 2.5 was reached.When the cells were standing idle, the rate of selfdischarge of each plate was determined by noting itspotential drop from day to day, the potential being measuredagainst a cadmium half cell. These readings were taken witha potentiometer, set-up, as illustrated in It'igure1.After remaining idle for a definite length of time, adischarge was made, using the arrangement as shown in ltigure2. The ampere hours obtained from each cell were utilizedto produce a deposit of copper in the coulometer. From this,the capacity was determined by calculation. A cellon thedischarge circuit was considered to be depleted of its energywhen a voltage of 1.8 was reached.RESULTS AND DISCUSSIONSIn the case of charging voltages, cells containing ironand manganese were expected to have potentials which differedfrom that of a normal cell. This expectation arose from thefact that these salts, being so easily oxidized and reduced,would tend to dissipate of the energy being delivered tothe cells, but on the contrary, no differences could bedetected. All cells were charged up to a line voltage of2.5 volts in the same length of time.The cell potentials and single potential of the platesdid not deviate much from those of a normal cell, even after-8-remaining idle for eight or ten days. The data taken duringsuch periods is recorded in the following table. In readingthis, it must be kept in mind that the cadmium half cell wasalways negative to the plates. Also, the "minus" s:i,gnasplaced before a figure indicates that the potential of thelead-cadmium or the lead dioxide-cadmium is becoming morenegative by this value. The "plus" sign applied in the samemanner, except that the change denotes the potential as onebecoming more negative.ImpurityConcentrationin grams of Cell Voltagemetal per liteT first dayof electrolyte afte,r chargeAverage dropin cellpotentialper dayVariation ofpotenti al ofcadmium to:Pb02Plate Pb PlateNone 2.1460 .0035 -.0043 -.0008Zinc .07395 2.1478 .0035 -.0043 -.0008Zinc .14790 2.14SS .0036 -.0045 -.0009Zinc .29580 2.1471 .0033 -.0039 ~.0006Zinc .36975 2.1443 .0030 -.0034 -.0004Zinc 7.395Q 2.1112 .0039 -.0032 +.0007Iron .014 2.1116 .0036 -.0030 +.OOOSIron .028 2,1042 .0037 -.0033 ••0004Manganese .020 2.1082 .0042 -,0036 +.OOOSManganese .040 2.1030 .0042 -.0035 +.0007-9-The potential change per day is slight, but it is inter-esting to note that this figure, with the first additionsof zinc, became smaller, and, then when the concentrationreached something near 0.5 grams of zinc per liter ofelectrolyte, it begins to increase. The potentials, thatwere taken each day, of the cadmium~sulphuric acid half cellagainst each plate indicates the effects of the differentconcentrations on the cell electrodes. With increasingconcentrations of zinc, the lead dioxide potential shows adecreasing tendency to become more negative with each succeed~ing day of idleness. The sponge lead potential, on the otherhand, moves in a more negative direction with the small con·centrations, but, as the concentration increases, the changeper day in this direction diminishes until a concentrationof about 0.5 grams of zinc per liter of electrolyte is reached,after which the potential of the sponge lead becomes morepositive with each day of idleness. Iron and manganese presentin any concentrations accelerated the natural tendency of thecathode to become more positive and the anode less positivewith each succeeding day of idleness. Therefore, these in-creased the average potential drop per day of their cellsas compared with that of a normal cell.The capacities of the cells were rather drasticallyaffected by iron, manganese and the high concentration of zinc.From statements made by "Arendtllt (Bibliography 3) the loss of-10....capacity was not expected to be so great. The cells, fromwhich the capacities recorded here were taken, remainedidle for twelve days; following this, they were discharged(s:et-upas in Figure 2). The ampere hours obtained fromeach cell was noted by the amount of copper they depositedin a coulometer. The percentage loss of capacity of anycell was determined .by comparison with a normal cell, thecapacity of which was assumed to be one hundred per cent.Concentration Ln Capacity in Percentage ofImpurity grams of metal per amperes per loss as comparedliter of electrolyte hour with normal cellNone 5.6 0Manganese .04 1.37 75.5Manganese .02 2.30 58.9Iron .028 2.53 54.8Iron •014 3.14. 43.9Zinc 7.395 2.52 55.0The voltage of these cells on discharge vary somewhataccording to their capacities, as shown by the accompanyingcurves, in which voltage is plotted as the abscissa and thehours of discharge as the ordinate.~~~Cfl s~H ttl~fir.t~0I ~ HiXtIJ::@H~~~~~N~~;~HI=l s~ H0JZ.rs§~~0CJ)HI=l-11-CONCLUSIONSFrom the foregoing discussion of this work, it isevident that every precaution possible was taken to getaccurate results. Such being the case, confidence is placedin the data so that the following conclusions may be drawnup:1. The impurities studied showed no effect on the voltagecharacteristics of a cell that is being charged.2. Zinc, added to a normal cell in concentrations smallerthan 0.5 grams per liter of electrolyte, is slightlybeneficial to it during its idle period, since it de-creases its potential drop per day. However, concen-trations larger than this are of no advantage. Inregard to capacity, there are no effects due to concen-trations smaller than 0.5 grams per liter of electrolyte,but, if this is boosted to something near seven grams,the loss of capacity from that of a normal cell is fiftyper cent. Evidently, then, this impurity is not desirablein any concentration above 0.5 grams per liter of electrolyte.3. Iron is definitely injurious to a battery if it is presentin any concentration. The data shows that in an idle cell0.01 grams of iron per liter of electrolyte causes anincrease in the potential drop per day. The capacity under-12~such conditions is lowered as much as forty-five per cent.4. Manganese is even more detrimental to a battery than isiron. It has an even greater tendency to increase thepotential drop per day of an idle cell over that of anormal cell. Also noticeable, is a more pronounced lossof capacity. Therefore, this impurity should never beallowed to enter a battery.ACKNOWLEDGMENTI wish to acknowledge the help andguidance that I have received from Dr. A. E. Koenigunder whose direction this work was done. I also wishto express my appreciation to Dr. C. L. Wilson andMr. J. U. MacEwan for their help and suggestions.-13-BIBLIOGRAPHY1. storage Batteries, Theory, Manufacture, Care andApplication. Morton Arendt Pages 43 - 48.2.. Cadmium Electrode for storage Battery Testing.W. J. Holmes and R. ElliotTrans. Am. Electrochem. Soc. Vol. LXII Page 2673. Storage Batteries, Theory, Manufacture, Care andApplication. Morton Arendt Page 82.4. Theory of the Lead Storage BatteryL. JumauTrans. Am. Electrochem. Soc. Vol. LIlI Page 245

The Effects of Zinc Sulphate, Manganese Sulphate, and Iron Sulphate on the Lead Storage Cell.

http://digitalcommons.mtech.edu/cgi/viewcontent.cgi?article=1057&context=bach_theses

The Effects of Zinc Sulphate, Manganese Sulphate, and Iron Sulphate on the Lead Storage Cell.

Abstract

Similar works

Full text

Available Versions

Digital Commons @ Montana Tech