Water is being electrolysed in the presence of a non-reactive electrolyte under standard conditions. If 2.5 amperes of current flows through the circuit for 13.6 minutes at 25 degrees celsius and 1 atmosphere, what volume of hydrogen gas is produced?

Please, I need help with this question. Thank You.

Oh, hydrogen gas production—we're really gassing things up here! Let's calculate it.

First, we need to find the number of moles of electrons that flow through the circuit. To do that, we use Faraday's constant, which is approximately 96,485 Coulombs per mole.

So, 2.5 amperes times 13.6 minutes gives us the total charge in Coulombs. Don't forget to convert minutes to seconds! Once we have the charge, we can divide it by the Faraday constant to get the number of moles of electrons.

Now that we have the number of moles of electrons, we can determine the number of moles of hydrogen gas produced. Since the reaction is 2H2O -> 2H2 + O2, the stoichiometry tells us that for every 2 moles of electrons, we get 1 mole of hydrogen gas.

Finally, we just need to use the Ideal Gas Law to find the volume of hydrogen gas. Since we're under standard conditions, we can use the molar volume of a gas at STP, which is 22.4 L/mol. Multiply this by the number of moles of hydrogen gas, and voila! You'll have the volume of hydrogen gas produced in liters.

I hope my electrifying explanation helps!

To find the volume of hydrogen gas produced, we need to use Faraday's law of electrolysis.

Faraday's law states that the amount of substance produced or consumed during electrolysis is directly proportional to the charge passed through the electrolyte. The formula to calculate the amount of substance produced or consumed is:

n = Q / (zF)

Where:
n is the number of moles of substance produced or consumed,
Q is the charge passed through the electrolyte in Coulombs (C),
z is the number of electrons transferred during the reaction, and
F is Faraday's constant, which is 96,485 C/mol.

In this case, we are interested in the volume of hydrogen gas produced. Since hydrogen gas is diatomic, 2 moles of electrons are required for each mole of hydrogen gas produced (z = 2).

First, we need to calculate the charge passed through the electrolyte (Q) using the formula:

Q = I * t

Where:
I is the current in Amperes (A),
t is the time in seconds (s).

Given:
I = 2.5 A
t = 13.6 minutes = 13.6 * 60 = 816 seconds

Q = 2.5 A * 816 s = 2040 C

Now we can calculate the number of moles of hydrogen gas produced (n):

n = Q / (zF) = 2040 C / (2 * 96485 C/mol) = 0.0106 moles

Since one mole of any gas occupies 22.4 liters at standard conditions, we can calculate the volume of hydrogen gas produced:

Volume = n * 22.4 L/mol = 0.0106 moles * 22.4 L/mol = 0.238 L

Therefore, the volume of hydrogen gas produced is 0.238 liters.

To find the volume of hydrogen gas produced, we need to use Faraday's law of electrolysis, which states that the amount of substance produced during electrolysis is directly proportional to the electric current passed through the electrolyte and the time of electrolysis.

The equation we will use is:

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

Where:
n is the amount of substance produced (in moles)
I is the current (in amperes)
t is the time of electrolysis (in seconds)
F is Faraday's constant (96485 C/mol)
z is the number of electrons transferred per mole of substance (for hydrogen gas, z = 2)

First, let's convert the current from amperes to coulombs per second:
2.5 amperes = 2.5 coulombs per second

Next, let's convert the time from minutes to seconds:
13.6 minutes = 13.6 * 60 seconds = 816 seconds

Now we can substitute these values into the equation:

n = (2.5 * 816) / (96485 * 2)

Calculating this, we get:

n ≈ 0.021 moles

Since water consists of 2 moles of hydrogen gas per mole of water, the amount of hydrogen gas produced will be:

0.021 moles * 2 = 0.042 moles

Now we need to find the volume of hydrogen gas using the ideal gas law:

V = n * R * T / P

Where:
V is the volume of the gas (in liters)
n is the amount of substance (in moles)
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature (in Kelvin)
P is the pressure (in atmospheres)

Let's convert the temperature from degrees Celsius to Kelvin:

25 degrees Celsius = 25 + 273.15 Kelvin = 298.15 Kelvin

Now we can substitute all the values into the equation:

V = 0.042 * 0.0821 * 298.15 / 1

Calculating this, we get:

V ≈ 1.02 liters

Therefore, approximately 1.02 liters of hydrogen gas would be produced under the given conditions.

coulombs = amperes x seconds

2.5 A x 13.5 min x (60 sec/min) = about 2000 C (but you should do it more accurately)
2000C/96,485 = ?F
1 F will free 11.2 L hydrogen.