How many minutes does it take to form 10.0L of O2 Measured at 99.8kpa and 28 C from water if a current of 1.3A passes through the electrolytic cell? what mass of h2 forms?

To calculate the time required to form 10.0L of O2, we need to use Faraday's law of electrolysis. According to Faraday's law, the quantity of a substance formed at an electrode is directly proportional to the amount of charge passing through the electrolytic cell.

1. Calculate the number of moles of O2 required to form 10.0L of O2 at the given conditions:
- Convert the volume to the number of moles using the ideal gas law:
PV = nRT
n = PV / RT
- Given:
P = 99.8 kPa
V = 10.0 L
R = 8.314 J/(K*mol)
T = 28 + 273 = 301 K (convert to Kelvin)
- Calculate:
n = (99.8 * 10^3 Pa) * (10.0 * 10^(-3) m^3) / (8.314 J/(K*mol) * 301 K)

2. Calculate the amount of charge required to produce the calculated number of moles of O2:
- Use Faraday's law: Q = n * F
Q = charge (Coulombs)
n = number of moles
F = Faraday's constant = 96,485 C/mol (Coulombs/mole)
- Calculate:
Q = n * F

3. Determine the time required for 1.3A (Amperes) of current to pass through the electrolytic cell:
- The relationships between charge (Coulombs), current (Amperes), and time (seconds) is given by: Q = I * t
Q = charge (Coulombs)
I = current (Amperes)
t = time (seconds)
- Rearrange the equation to solve for time:
t = Q / I

4. Calculate the time required:
- Use the calculated charge from step 2 and the given current of 1.3A:
t = (Q / I)

5. Calculate the mass of H2 formed using the stoichiometry of the water electrolysis reaction:
- 2H2O -> 2H2 + O2
- The molar mass of H2 is 2 g/mol.
- The molar mass of O2 is 32 g/mol.
- Since the reaction produces 2 moles of H2 for every 1 mole of O2, the mass ratio is 2:1.
- Calculate the moles of H2 formed using the moles of O2 from step 1:
Moles of H2 = 2 * moles of O2
- Calculate the mass of H2 formed by multiplying the moles of H2 by the molar mass of H2.

Please provide the temperature of the water in the electrolytic cell so we can compute a more accurate answer.

To determine the time it takes to form 10.0L of O2 and the mass of H2 formed using an electrolytic cell, we need to consider Faraday's Laws of Electrolysis.

1. Calculate the moles of O2 formed:
We'll use the Ideal Gas Law, PV = nRT, where:
P = pressure (99.8 kPa),
V = volume (10.0 L),
n = moles of gas (oxygen),
R = ideal gas constant (0.0821 L·atm/mol·K),
T = temperature (28 °C = 301 K).

Rearranging the equation to isolate n, we have:
n = PV / RT

Substituting the values and converting pressure to atm:
n = (99.8 kPa * 1 atm/101.3 kPa) * (10.0 L) / (0.0821 L·atm/mol·K * 301 K)

Solving the equation yields the moles of O2.

2. Determine the time using Faraday's First Law of Electrolysis:
Faraday's Law states that the amount of substance produced or consumed in an electrolysis reaction is directly proportional to the quantity of electricity passed through the cell.

The equation to calculate the moles of O2 is:
moles of O2 = (current in amperes * time in seconds) / (Faraday constant * number of electrons per mole of O2)
The Faraday constant represents the charge of one mole of electrons (~96,485 C/mol).

Rearranging the equation to solve for time:
time = (moles of O2 * Faraday constant * number of electrons per mole of O2) / current

Substitute the values, including the moles of O2 from step 1, to calculate the time in seconds.

3. Calculate the mass of H2 formed:
We need to apply the same principles used in step 2, but this time for H2.
The balanced equation for the formation of H2 is: 2H2O(l) -> 2H2(g) + O2(g)

Use the stoichiometry of the reaction to determine the number of moles of H2 produced.
For every 1 mole of O2, 2 moles of H2 are produced.

Multiply the moles of O2 obtained in step 1 by the stoichiometric ratio to get moles of H2.
Multiply the moles of H2 by its molar mass (2.02 g/mol) to get the mass of H2 formed.

By following these steps, you can determine both the time it takes to form 10.0L of O2 and the mass of H2 formed using the given conditions and information.