The amount of HHO gas (a mixture of hydrogen and oxygen) produced by an electrolysis cell depends on various factors, including the efficiency of generator, the surface area of the electrodes, and the quality of the water. However, here is the rough estimate.
When we run electrolysis on 1 liter of distilled water using 12 volts and 1 ampere, we are providing a power of 12 watts (12 volts * 1 ampere). The efficiency of the process can vary, but let’s assume a reasonable efficiency of around 70%.
So, 70% of 12 watts is 8.4 watts available for the electrolysis reaction. Now, to calculate the amount of gas produced, we can use the ideal gas law, which relates the amount of gas produced to the power input:
PV = nRT
Where:
P = pressure (usually at standard atmospheric pressure)
V = volume (in liters)
n = moles of gas
R = universal gas constant
T = temperature (in Kelvin)
At standard temperature and pressure (STP), which is 0 degrees Celsius and 1 atmosphere of pressure, 1 mole of any gas occupies approximately 22.4 liters.
Assuming the gas produced is primarily hydrogen (H2), the molar mass of hydrogen is about 2 grams/mol.
Now, let’s calculate:
8.4 watts = 8.4 joules/second (since 1 watt = 1 joule/second)
Let’s assume the gas is produced at STP (0 degrees Celsius, 1 atmosphere of pressure).
So, n = (8.4 joules/second) / [(22.4 liters/mol) * (2 grams/mol) * (1/1000 kg/gram)] = 0.015 moles of hydrogen gas per second.
Now, if we want to know how much gas is produced in 1 liter of distilled water over 1 hour (3600 seconds), we can multiply:
0.015 moles/second * 3600 seconds = 54 moles of hydrogen gas
At STP, 1 mole of any gas occupies 22.4 liters, so:
54 moles * 22.4 liters/mole = 1,209.6 liters of hydrogen gas
Keep in mind that this is a simplified calculation, and real-world conditions may result in different values based on the efficiency of your generator and other factors. Additionally, safety precautions should be taken when working with hydrogen gas, as it is flammable and can be hazardous if not handled properly.