a current of .500 A is used for the electrolytic decomposition of water. how long (in hours) will it take to produce 1.0 L (Standard temperature and pressure) of hydrogen gas? what mass of oxygen gas will be produced at the same time?

2H2O ==> 2H2 + O2

amp x seconds = coulombs.
96,485 coulombs will deposit 1 g H atoms or
2*96,485 coulombs will deposit 2g H2 molecules which will occupy 22.4L at STP.
Coulombs for 1.0L will be
2*96,485 x (1.0/22.4) = about8615 (approximately) ,then
amps x sec = about 8615, substitute for amps, solve for sec and convert to min then to hours. From the equation you can see that 2 mol H2 will be produced for every mole of O2 produced; therefore, or 4 g hydrogen for every 32 O2. So take grams H2 x (32/4) = ?

To determine the time it takes to produce 1.0 L of hydrogen gas and the mass of oxygen gas produced, we need to use Faraday's laws of electrolysis.

First, we need to calculate the amount of charge (Q) required to produce the desired quantity of hydrogen gas. The equation Q = It relates charge (Q), current (I), and time (t), where I is the current and t is the time. Rearranging the equation, we have t = Q/I.

Next, we need to determine the amount of charge required to produce one mole of hydrogen gas. According to Faraday's laws of electrolysis, the charge required to produce one mole (2 grams) of any substance during electrolysis is 96,485 Coulombs (C). This value is known as the Faraday constant (F).

Now, let's calculate:

1. Determine the amount of charge required to produce 1.0 L of hydrogen gas:
- The molar volume of any gas at standard temperature and pressure (STP) is 22.4 L/mol.
- As hydrogen gas has a molar mass of 2 g/mol, 1.0 L of hydrogen gas corresponds to 1.0/22.4 = 0.04464 moles of hydrogen gas.
- Therefore, the charge required is Q = 0.04464 * 96,485 C.

2. Calculate the time required to produce the given amount of hydrogen gas:
- Using the formula t = Q/I, substitute the values Q = 0.04464 *96,485 C and I = 0.500 A.
- t = (0.04464 * 96,485 C) / 0.500 A.

Finally, to find the mass of oxygen gas produced, we use the fact that water undergoes electrolysis in a 2:1 ratio of hydrogen to oxygen by moles. Therefore, if 0.04464 moles of hydrogen gas is produced, we will have 0.04464 * 2 = 0.08928 moles of oxygen gas produced.

To calculate the mass of oxygen gas:
- The molar mass of oxygen gas is 32 g/mol.
- Multiply the moles of oxygen gas by its molar mass to get the mass.

That's how you can calculate the time to produce 1.0 L of hydrogen gas and the mass of oxygen gas produced during electrolysis.