Electrochemistry
LEC 06
Determination of Faraday’s constant 06.21 What you can learn about Electrolysis Coulometry Faraday’s laws
Principle and tasks The correlation between the amounts of substances transformed in the electrode reaction and the applied charge is described by Faraday’s laws. Faraday’s constant, which appears as a proportionality factor, can be determined experimentally, in this case from the dependence of the volumes of hydrogen and oxygen evolved on the applied charge in the hydrolysis of diluted sulphuric acid.
What you need: Power supply, universal Digital multimeter Electrolysis apparatus after Hofmann Platinum electrode, protective sleeve, d = 8 mm On/Off switch Connecting cord, l = 250 mm, red Connecting cord, l = 500 mm, red Connecting cord, l = 750 mm, blue Retort stand, h = 750 mm Right angle clamp Universal clamp Stopwatch, digital, 1/100 s Weather monitor, LCD Precision balance CPA 623S (620 g/0.001 g), set with software Beaker, 600 ml, short Funnel, glass, do = 80 mm Pasteur pipettes Rubber bulbs Wash bottle, 500 ml Sulphuric acid, 95…98 %, 500 ml Water, distilled, 5 l
13500.93 07128.00 44518.00 45206.00 06034.01 07360.01 07361.01 07362.04 37694.00 37697.00 37715.00 03071.01 87997.10
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49224.88 36015.00 34459.00 36590.00 39275.03 33931.00 30219.50 31246.81
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Determination of Faraday’s constant P3062101 PHYWE Systeme GmbH & Co. KG · D - 37070 Göttingen
Laboratory Experiments Chemistry 91