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2 THE MANUFACTTJBE OF CHEMICALS BY ELECTKOLYSIS a continuous current of electricity at a pressure of about 2 volts between metal electrodes immersed in the solution, a definite volume of hydrogen is liberated at one electrode, and half the volume of oxygen at the opposite electrode. That electrode at which the hydrogen is discharged is known as the cathode, and is connected with the negative pole of the battery or machine supplying the current. The electrode at which oxygen is discharged is the anode, and is connected with the positive pole of the current source. The decomposition voltage necessary for decomposing water by electrolysis can be calculated from the heat of formation which is 68,400 calories. Since 1 joule or 1 volt-coulomb *is equivalent to 0'239 calorie, the electrical energy necessary for decomposing 1 gram-molecule of 68400 water will be .^QQ =• 285,714 volt-coulombs. Two equi- of hydrogen will be discharged, and this amount will require, according to Faraday's Law, 2 x 96500 coulombs of electricity ; the voltage necessary for decom- OQKrr-| A = position will therefore be ^ 96500 1*48 volts. Owing to various conductivity losses the voltage needed between the electrodes in the various forms of plant varies from 1*9 to as much as 4 volts. The solutions generally employed are dilute sulphuric acid (10-20 per cent.) or dilute alkali solution containing potassium or sodium hydroxide, and sometimes potassium carbonate is utilised (10-25 per cent.). 1 See Appendix*PDF Image | MANUFACTURE OF CHEMICALS BY ELECTROLYSIS
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