How many minutes does it take to produce 10.0L of oxygen gas (at standard conditions)
by electrolyzing neutral water with a current of 1.3 A? What is the corresponding volume
of hydrogen gas produced?
thanks so much
2H2O ==> 2H2 + O2
10.0 L O2 at STP = 10/22.4 mols = 0.446 mols or 0.446 x 32 = 14,3 grams O2.
96,485 coulombs will produce 32/4 = 8 g O2 so
coulombs needed = 96,485 x (14.3/8) = ?
Coulombs = amperes x seconds = 1.3*seconds. Plug in coulombs and A and solve for seconds. Convert to minutes. Post your work if you get stuck.
To determine the time required to produce 10.0L of oxygen gas and the corresponding volume of hydrogen gas produced by electrolyzing neutral water with a current of 1.3 A, we need to use Faraday's law of electrolysis.
Faraday's law states that the amount of a substance produced or consumed during electrolysis is directly proportional to the quantity of electric charge passed through it.
The equation for Faraday's law is:
m = (I * t) / (n * F)
where:
m is the mass of the substance (in this case, oxygen or hydrogen gas)
I is the current (in amperes)
t is the time (in seconds)
n is the number of moles of electrons (in this case, 4 moles of electrons for each mole of oxygen gas and 2 moles of electrons for each mole of hydrogen gas)
F is Faraday's constant, which is approximately equal to 96,485 Coulombs/mol
First, let's find the time required to produce 1 mole of oxygen gas using the given current of 1.3 A:
n = 4 moles of electrons
I = 1.3 A
F = 96,485 C/mol
Rearranging the equation, we have:
t = (m * n * F) / I
Substituting the values for m (1 mole), n (4 moles), I (1.3 A), and F (96,485 C/mol), we can find the time required to produce 1 mole of oxygen gas.
t = (1 * 4 * 96,485) / 1.3
To determine the time required to produce 10.0 L of oxygen gas, we need to multiply the time calculated above by 10.0:
t required = t * 10.0
Next, we need to find the volume of hydrogen gas produced. Since oxygen gas and hydrogen gas are produced in a 2:1 ratio during electrolysis of water, the volume of hydrogen gas produced will be half of the volume of oxygen gas produced.
Now that we have the time required to produce 10.0 L of oxygen gas, we can calculate the corresponding volume of hydrogen gas.
Volume of hydrogen gas = (1/2) * Volume of oxygen gas
You can now substitute the value of time required to produce 10.0 L of oxygen gas into the equation to find the corresponding volume of hydrogen gas.
Please note that the given conditions are assumed to be at standard temperature and pressure (STP) for this calculation.