How long does it take to produce H2 in a closed beaker

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SUMMARY

The discussion focuses on calculating the time required to produce hydrogen gas (H2) in a closed beaker with a volume of 5 liters, pressure of 10 MPa, and temperature of 20°C, using an electric current of 0.7A. The participant calculated approximately 20.515 moles of hydrogen gas based on ideal gas behavior. The key inquiry is about the formula or method to determine the time needed for electrolysis to produce this amount of hydrogen gas at the specified current.

PREREQUISITES
  • Understanding of electrolysis principles
  • Knowledge of the ideal gas law
  • Familiarity with Faraday's laws of electrolysis
  • Basic electrical concepts related to current and moles
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  • Research Faraday's laws of electrolysis to calculate the time for hydrogen production
  • Learn about the ideal gas law and its application in electrolysis
  • Explore the relationship between current, moles, and time in electrochemical reactions
  • Investigate practical electrolysis setups and their efficiency
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Chemistry students, electrochemists, and anyone involved in hydrogen production or electrolysis processes.

PeetPb
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hi,
I've got a problem which I cannot solve. The problem says that How long does it take to produce H2 in a closed beaker with volume 5l pressure 10Mpa and temp. 20 C with a current of 0.7A. First thing I did was to calculate the amount of H2 in that beaker. Assuming that it behaves ideally I calculated that there should be about 20.515 moles of hydrogen. And what now ? Is there any formula for this ?
thanx
 
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How fast can you produce the hydrogen gas with a 0.7A current?
 


what's the time needed for electrolysis to produce that amount of H2
 

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