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How can i calculate the amount of hydrogen generated and needed per volt & watt of an electrolysis device for hydrogenation and how much hydrogen is generated via electrolysis at 100v 1a and provide me with an example for the electrohydrogenation of a known substance?
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1) Calculating the amount of hydrogen generated and needed per volt & watt of an electrolysis device for hydrogenation
The amount of hydrogen generated per volt and watt of an electrolysis device can be calculated using Faraday's law of electrolysis. This law states that the amount of substance produced at an electrode during electrolysis is directly proportional to the amount of charge passed through the electrode.
The amount of charge passed through an electrode is given by the equation:
Q = I * t
where Q is the charge in coulombs, I is the current in amps, and t is the time in seconds.
The amount of substance produced at an electrode is given by the equation:
m = Q / (z * F)
where m is the mass of the substance in grams, z is the number of electrons transferred per mole of the substance, and F is the Faraday constant (96,485 C/mol).
For hydrogen, z = 2, and F = 96,485 C/mol.
Therefore, the amount of hydrogen generated per volt and watt of an electrolysis device can be calculated using the following equation:
m = (I * t) / (2 * 96,485)
where m is the mass of hydrogen in grams, I is the current in amps, and t is the time in seconds.
2) Calculating the amount of hydrogen generated via electrolysis at 100v 1a
Using the equation above, we can calculate the amount of hydrogen generated via electrolysis at 100v 1a.
m = (1 * t) / (2 * 96,485)
m = 0.0051 g/s
Therefore, the amount of hydrogen generated via electrolysis at 100v 1a is 0.0051 g/s.
3) Example of the electrohydrogenation of a known substance
One example of the electrohydrogenation of a known substance is the hydrogenation of ethene to ethane. This reaction can be carried out in an electrochemical cell with a platinum cathode and a nickel anode. The ethene is bubbled through the cell, and the hydrogen is generated at the cathode.
The overall reaction for the electrohydrogenation of ethene is:
C2H4 + H2 → C2H6
The amount of hydrogen generated per volt and watt of an electrolysis device can be calculated using Faraday's law of electrolysis. This law states that the amount of substance produced at an electrode during electrolysis is directly proportional to the amount of charge passed through the electrode.
The amount of charge passed through an electrode is given by the equation:
Q = I * t
where Q is the charge in coulombs, I is the current in amps, and t is the time in seconds.
The amount of substance produced at an electrode is given by the equation:
m = Q / (z * F)
where m is the mass of the substance in grams, z is the number of electrons transferred per mole of the substance, and F is the Faraday constant (96,485 C/mol).
For hydrogen, z = 2, and F = 96,485 C/mol.
Therefore, the amount of hydrogen generated per volt and watt of an electrolysis device can be calculated using the following equation:
m = (I * t) / (2 * 96,485)
where m is the mass of hydrogen in grams, I is the current in amps, and t is the time in seconds.
2) Calculating the amount of hydrogen generated via electrolysis at 100v 1a
Using the equation above, we can calculate the amount of hydrogen generated via electrolysis at 100v 1a.
m = (1 * t) / (2 * 96,485)
m = 0.0051 g/s
Therefore, the amount of hydrogen generated via electrolysis at 100v 1a is 0.0051 g/s.
3) Example of the electrohydrogenation of a known substance
One example of the electrohydrogenation of a known substance is the hydrogenation of ethene to ethane. This reaction can be carried out in an electrochemical cell with a platinum cathode and a nickel anode. The ethene is bubbled through the cell, and the hydrogen is generated at the cathode.
The overall reaction for the electrohydrogenation of ethene is:
C2H4 + H2 → C2H6
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