Clifton College Scientific Society. 81 



peculiar odour, oxidizes ammonia (NII3), and causes the less 

 inflammable varieties of phospliuretted hydrogen (PH3 con- 

 taining minute quantities of PsHjo (PH,,) and P2H in suspen- 

 sion). ' Later researches have, however,' says the late Prof, 

 Miller, ' rendered it probable that these properties are due 

 to the formation of peroxide of hydrogen in small quantity, 

 and to its suspension in the oxygen as it escapes.' {Elem. 

 Chem. ii. 338.) 



(9) By the galvanic decomposition of dilute sulphuric acid 

 (HjSO^ajHjO) or a solution of the sulphates (M'jSOj, chro- 

 mates (M'/CrOj, phosphates (M'jPO,, M'^HPO, or M'H^PO,), 

 and other salts of the alkalis between poles of gold and 

 platinum. 



(10) 'By rubbing with a pestle in a mortar, or in water, or 

 wiih carbonate of potassium (KgCOj), a blackish violet- 

 coloured fluor spar (CaF2) called Chlorophane. "When a 

 strong odour of hypochlorous acid (HCIO) or ozone is evolved, 

 hypochlorous acid and any other possible substances of the 

 like character have been proved by Schrotter to be absent 

 and ozone only present. 



(11) When finely divided platinum and certain other 

 metals are slowly oxidizing ozone and peroxide of hydrogen 

 (H2O2) are evolved. 



(12) Several hydrocarbons ozonize air when exposed to 

 sunlight. 



(18) The oxidation of several substances in moist air — 

 such as oil of bitter almonds (C^HgO), sulphurous acid (SO2), 

 phosphorous acid (P2O3), oil of tiu-pentine {C^QH.^g), stibethyl 

 SbCgH,3), phosphorus, &c. The latter substance is the most 

 convenient for manipulation. The operation may be con- 

 ducted as follows: — Take a piece of clean scraped phospho- 

 rus (an exceedingly convenient method of cleaning the 

 outside of the phosphorus is to melt it in a test tube under 

 water, allow it to cool, and remove by breaking away the test- 

 tube) ; place the stick of phosphorus at the bottom of a 

 wide-mouthed jar, pour in water in sufficient quantity to 

 cover half the phosphorus, cover the mouth of the jar with a 

 glass plate, and allow it to stand in a temperature of from 

 60° to 70° F. (15° to 21° C) for about two hours, by whicli 

 time the oxidation of the phosphorus will have been attended 

 Avith the production of ozone. If the phosphorus is not 

 now removed, it will recombine with the newly formed ozone, 

 and thus destroy it. The formation of ozone will be rendered 

 evident by the light luminous column of smoke which rises 

 from the phosphorus, and is due to the formation of ammo- 



G 



