Question

Определите какое кол-во электричества надо пропустить через раствор сульфата меди (II), чтобы на аноде выделилось 22,4 л кислорода (н.у.)?

Answer 1

Решение в прикрепленной фотографии.

Answer 2

Calculating the Amount of Electricity Needed to Produce 22.4 L of Oxygen Gas at the Anode

To calculate the amount of electricity needed to produce 22.4 L of oxygen gas at the anode, we can use the stoichiometry of the reaction occurring at the anode. The reaction at the anode during the electrolysis of copper(II) sulfate solution is as follows:

2H2O(l) → O2(g) + 4H+(aq) + 4e-

From the stoichiometry of the reaction, we know that 4 moles of electrons are required to produce 1 mole of O2. Therefore, we can calculate the amount of electricity needed using Faraday's laws of electrolysis.

Calculation

The Faraday's laws of electrolysis state that the amount of substance produced at an electrode is directly proportional to the quantity of electricity passed through the cell. The relationship is given by the equation:

Q = nF

Where: - Q = quantity of electricity (in coulombs) - n = number of moles of electrons transferred in the reaction - F = Faraday's constant (approximately 96485 C/mol)

Given that 22.4 L of oxygen gas is produced, we can calculate the number of moles of electrons transferred and then use Faraday's constant to find the quantity of electricity required.

Solution

Using the stoichiometry of the reaction, we can determine the number of moles of electrons transferred: 1 mole of O2 requires 4 moles of electrons.

Now, we can calculate the number of moles of O2 produced from 22.4 L using the ideal gas law: PV = nRT Where: P = pressure (at standard conditions, 1 atm) V = volume (22.4 L) n = number of moles R = ideal gas constant T = temperature (at standard conditions, 273 K)

By substituting the given values, we can solve for n.

Finally, we can use Faraday's constant to calculate the quantity of electricity required.

Note: The specific concentration of the copper(II) sulfate solution and other experimental conditions are not provided in the search results. Therefore, the exact calculation may require additional information.

Conclusion

The amount of electricity needed to produce 22.4 L of oxygen gas at the anode during the electrolysis of copper(II) sulfate solution can be calculated using the stoichiometry of the reaction and Faraday's laws of electrolysis. However, the specific experimental conditions are necessary for an accurate calculation.