How many minutes does it take to form 10L of O2 measured at 92.2 kPa and 28°c from water if a current of 1.3 A passes through the electolytic cell?

a) how many minutes?

b)What mass in grams of h2 forms?

To determine the amount of time it takes to form 10L of O2 from water in an electrolytic cell, we need to use the concept of Faraday's laws of electrolysis.

Faraday's first law states that the amount of substance formed or consumed during an electrolysis reaction is directly proportional to the quantity of electricity (charge) passing through the cell.

We can use the formula:

n = Q / F

Where:
n = number of moles of substance formed or consumed
Q = quantity of electricity (charge) passed through the cell
F = Faraday's constant (96485 C/mol)

Now let's calculate the number of moles of O2 formed:

Step 1: Convert 10L of O2 to moles using the ideal gas law.

PV = nRT

P = 92.2 kPa = 92.2 * 10^3 Pa
V = 10 L = 10 * 10^-3 m^3
R = ideal gas constant = 8.314 J/(mol·K)
T = 28°C = 28 + 273.15 K

n (moles) = (P * V) / (R * T)

Step 2: Calculate the quantity of electricity passed through the cell using the formula:

Q = I * t

Where:
Q = quantity of electricity (charge) passed (Coulombs)
I = current (Amperes)
t = time (in seconds)

We can convert minutes to seconds by multiplying by 60. Let's assume the given time is in minutes.

Now we can rearrange the formula to solve for time:

t = Q / I

Let's calculate the time it takes using the given current of 1.3 A:

t = Q / I
t = (n * F) / I

a) To calculate the time in minutes, we also need to convert the time to minutes by dividing by 60.