Question

Электролиз раствора сульфата натрия проводили в течение 5 ч, в результате чего выделилось 6 л кислорода, измеренного при н. у. Вычислите силу тока. Составьте электронные уравнения процессов, происходящих на электродах.

Answer 1

Electrolysis of Sodium Sulfate Solution

To calculate the current strength in the electrolysis of a sodium sulfate solution, we need to use Faraday's laws of electrolysis. Faraday's first law states that the amount of substance produced or consumed during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte. Faraday's second law states that the amount of substance produced or consumed during electrolysis is directly proportional to the equivalent weight of the substance.

In this case, we know that 6 liters of oxygen gas (O2) were produced during the electrolysis. To calculate the current strength, we need to determine the number of moles of oxygen gas produced and the amount of electricity passed through the electrolyte.

Calculation of Moles of Oxygen Gas Produced

To calculate the number of moles of oxygen gas produced, we can use the ideal gas law equation:

PV = nRT

Where: P = pressure (atmospheres) V = volume (liters) n = number of moles R = ideal gas constant (0.0821 L·atm/mol·K) T = temperature (Kelvin)

Since the volume of oxygen gas produced is given as 6 liters, we can substitute the values into the equation:

(1 atm) * (6 L) = n * (0.0821 L·atm/mol·K) * (273 K)

Simplifying the equation, we find:

6 = n * 22.414

n = 6 / 22.414

n ≈ 0.268 moles of oxygen gas

Calculation of Electricity Passed

To calculate the amount of electricity passed through the electrolyte, we can use Faraday's laws of electrolysis. According to Faraday's first law, the amount of substance produced or consumed during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.

The equation relating the amount of substance produced or consumed (n) to the quantity of electricity (Q) is:

n = Q / F

Where: n = number of moles Q = quantity of electricity (coulombs) F = Faraday's constant (96,485 C/mol)

We know that 0.268 moles of oxygen gas were produced. Substituting the values into the equation, we can solve for the quantity of electricity passed:

0.268 = Q / 96,485

Q = 0.268 * 96,485

Q ≈ 25,878.68 coulombs

Calculation of Current Strength

To calculate the current strength (I), we can use the equation:

I = Q / t

Where: I = current strength (amperes) Q = quantity of electricity (coulombs) t = time (seconds)

We know that the electrolysis was conducted for 5 hours, which is equivalent to 5 * 60 * 60 = 18,000 seconds. Substituting the values into the equation, we can solve for the current strength:

I = 25,878.68 / 18,000

I ≈ 1.437 amperes

Therefore, the current strength in the electrolysis of the sodium sulfate solution is approximately 1.437 amperes.

Electron Equations at the Electrodes

During the electrolysis of a sodium sulfate solution, the following processes occur at the electrodes:

At the anode (positive electrode): 2H2O(l) -> O2(g) + 4H+(aq) + 4e- At the cathode (negative electrode): 2H+(aq) + 2e- -> H2(g) Therefore, at the anode, water molecules are oxidized to produce oxygen gas, protons (H+ ions), and electrons. At the cathode, protons and electrons combine to form hydrogen gas.

Please note that the equations provided are simplified representations of the overall processes occurring during electrolysis and may not include all possible reactions that could occur in the electrolyte.

I hope this helps! Let me know if you have any further questions.