. The principles of chemistry . (salt) with it. Thus bariumperoxide, when heated with sulphuric acid, forms oxygen and bariumoxide, which gives a compound with sulphuric acid termed bariumsulphate (BaO.^ + = BaS04 + H^O -\- O).- ^i^ This reaction usually 9 We shall afterwards see that it is only substances like barium peroxide (whichgive hydrogen peroxide) which should be counted as true peroxides, and that MnO.,, PbOo,.&c., should be distinguished from them (they do not give hydrogen peroxide with acids),and therefore it is best to call them dioxides. 9 bis Peroxide of barium also give
. The principles of chemistry . (salt) with it. Thus bariumperoxide, when heated with sulphuric acid, forms oxygen and bariumoxide, which gives a compound with sulphuric acid termed bariumsulphate (BaO.^ + = BaS04 + H^O -\- O).- ^i^ This reaction usually 9 We shall afterwards see that it is only substances like barium peroxide (whichgive hydrogen peroxide) which should be counted as true peroxides, and that MnO.,, PbOo,.&c., should be distinguished from them (they do not give hydrogen peroxide with acids),and therefore it is best to call them dioxides. 9 bis Peroxide of barium also gives oxygen at the ordinary temperature in the presence IGO PRINCIPLES OF CHEMISTRY proceeds with greater ease than the decomposition of peroxides by heatalone. For the purposes of experiment powdered manganese peroxide isusually taken and mixed with strong sulphuric acid in a flask, and theajDparatus set up as shown in Fig. 28. The gas which is evolved ispassed through a Woulfes bottle containing a solution of caustic potash,. Pi(j. 28. Preparation of oxygen from manganese peroxiile and sulphuric acid. The gas evolved is passed through a Woulfes bottle containing caustic potash. to purify it from carbonic anhydride and chlorine, which accompany theevolution of oxygen from commercial manganese peroxide, and the gas isnot collected until a thin smouldering taper placed in front of the escapeorifice bursts into flame, which shows that the gas coming offis this method of decomposition of the manganese peroxide hj sul- of the solutions of many substances in a higher degree of oxidation. In this respect wemay mention that Kassner (1890) proposes to obtain oxygen for laboratory purposes with FeK^lCNle (red prussiate of i^otash, Chapter XXII.): the reactionproceeds with the evolution of oxygen even on the addition of a very small quantity ofwater. In order to ensure a gradual evolution of gas the author proposes to introducebotli substances into the reaction, lit
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