CHLORINE 83 



For the preparation of chlorine gas, the peroxide of man- 

 ganese is more economical than red lead. Place about 50 

 grams in the flask A (Fig. 35), pour in some 

 commercial hydrochloric acid (the impuri- 

 ties, viz. ferric chloride and sulphuric acid, 

 cannot interfere with the reaction), mix 

 thoroughly, and warm very gently. Pass the 

 escaping gas through water in B, and collect 

 some bottles of chlorine gas by downward y\g. 36. 



displacement of air. Then pass the gas into 

 a flask of cold water and prepare a saturated solution of 

 chlorine. The experiment must be conducted in a fume 

 chamber, as chlorine gas is highly injurious to inhale. 



Note the colour and smell of chlorine. Insert a jet of 

 burning hydrogen into one of the bottles. Note that the gas 

 is incapable of being set fire to in the air, but that it supports 

 the combustion of hydrogen with production of white fumes. 

 Is hydrochloric acid the product of combustion? Let the 

 fumes dissolve in a little water shaken in the bottle, blow air 

 through the solution till free from chlorine, and test for the acid 

 with blue litmus paper, and also with silver nitrate 

 solution. In another bottle of the gas place a glowing 

 splint. Is chlorine able to support the combustion of 

 ignited carbon? Now thrust a lighted taper into the 

 gas. Note the formation of the fumes of hydrochloric 

 acid and the liberation of carbon, the paraffin wax of 

 the taper being a compound of hydrogen and carbon. 

 Ignite some metallic sodium in an iron deflagrating 

 spoon, and place in another jar of the gas. What 

 is the product of combustion? As a result of these 

 experiments state whether chlorine is able to unite 

 directly with oxygen, hydrogen, carbon, or sodium. 



Fill a long glass tube, closed at one end, with the 

 saturated chlorine water, and invert it into a small wide- 

 necked flask also filled with the chlorine water. Slip a 



