How many grams of hydrogen can be produced by the electrolysis of water with a current of 0.442 A running for 2.00 min?

I got 0.000549g. can someone check my answer

I think what you have is 0.000549 g H but since hydrogen is diatomic, that will be 0.000549/2 g H2.

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To calculate the number of grams of hydrogen produced by electrolysis, you will need to use Faraday's law of electrolysis. This law states that the amount of substance produced or consumed during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.

First, we need to calculate the amount of charge (Q) passed through the electrolyte. The formula to calculate charge is:

Q = I * t

Where:
Q = Charge (in Coulombs)
I = Current (in Amperes)
t = Time (in seconds)

In this case, the current (I) is given as 0.442 A, and the time (t) is given as 2.00 min (or 120 seconds). Therefore, we can calculate the charge (Q) as follows:

Q = 0.442 A * 120 s
Q = 53.04 Coulombs

Next, we need to convert the charge (Q) from Coulombs to moles of electrons (n) using Faraday's constant (F), which is approximately 96,485 Coulombs per mole:

n = Q / F

n = 53.04 C / 96,485 C/mol
n = 0.000549 mol

Since the electrolysis of water involves the formation of 2 moles of hydrogen gas (H2) for every mole of electrons passing through, we can multiply the number of moles of electrons (n) by 2 to get the number of moles of hydrogen gas produced (m):

m = 2 * n
m = 2 * 0.000549 mol
m = 0.001098 mol

Finally, we can convert the moles of hydrogen gas (m) to grams using the molar mass of hydrogen (approximately 2.016 g/mol):

Mass of hydrogen = m * molar mass
Mass of hydrogen = 0.001098 mol * 2.016 g/mol
Mass of hydrogen = 0.002213 g

So, the correct answer is approximately 0.002213 grams of hydrogen. Therefore, your initial answer of 0.000549 g is incorrect.