Chemical Forums
Specialty Chemistry Forums => Chemical Engineering Forum => Topic started by: Fav123 on November 14, 2018, 11:07:06 AM
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Hello,
I need to determine the current required to produce dihydrogen in electrolysis of water. The production of hydrogen must be of 100t a day (1157.41 g/s). The potential difference in the electrodes is 2V. I need to find the current required for such a production, but when I do the maths, I find a very high current intensity. Can someone help me ?
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Faraday's laws of electrolysis are all you need.
High currents are nothing surprising in this context.
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Hello,
I need to determine the current required to produce dihydrogen in electrolysis of water. The production of hydrogen must be of 100t a day (1157.41 g/s). The potential difference in the electrodes is 2V. I need to find the current required for such a production, but when I do the maths, I find a very high current intensity. Can someone help me ?
It will be 115000 kA. What means bz using 2 V = 230000 kW = 230 MW . You need a power plant for that.
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Thank you very much for your help.
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Electricity is an expensive form of energy, most often obtained from heat, and electrolysis wastes much of the electric power. If electrolysis consumes 230MW, one should consider other ways to produce the hydrogen. Several paths exist, approximately like reacting a metal with water and reducing the metal oxide with heat (I've forgotten the details and may be inaccurate here).