Question

Пожалуйста решите.Составьте электронные уравнения процессов, происходящих на угольных электродах при электролизе раствора AgNO3. Если электролиз проводить с серебряным анодом, то его масса уменьшается на 5,4гр. Определите расход электричества при этом.

Answer 1

На угольных электродах: на катоде: Ag+ + 1e → Ag
на аноде: 2H2O - 4e → O2 + 4H+
В случае серебряного анода: Ag - 1e → Ag+
По закону Фарадея m(Ag) = Mэ(Ag) * Q / F отсюда Q = m(Ag) * F / Mэ(Ag) = 5.4 * 96500 / 108 = 4825 Кл

Answer 2

Electrolysis of AgNO3 Solution on Carbon Electrodes

During the electrolysis of a solution of AgNO3 (silver nitrate) using carbon electrodes, several processes occur at the anode and cathode. Let's break down the reactions and calculate the electricity consumption based on the given information.

Anode (Oxidation):

At the anode (positive electrode), the following reaction takes place: 2Ag(s) → 2Ag+(aq) + 2e- [[1]]

This reaction involves the oxidation of solid silver (Ag) to silver ions (Ag+) in the solution. Since the anode is made of silver in this case, it will dissolve as silver ions are formed. This explains the decrease in mass of the silver anode.

Cathode (Reduction):

At the cathode (negative electrode), the following reaction occurs: 2H2O(l) + 2e- → H2(g) + 2OH-(aq) [[2]]

In this reaction, water molecules (H2O) are reduced to hydrogen gas (H2) and hydroxide ions (OH-) in the solution.

Overall Reaction:

The overall reaction during the electrolysis of AgNO3 solution can be represented as: 2Ag(s) + 2H2O(l) → 2Ag+(aq) + H2(g) + 2OH-(aq)

Calculation of Electricity Consumption:

To determine the electricity consumption during the electrolysis process, 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.

The charge (Q) passed through the electrolyte can be calculated using the formula: Q = I * t where Q is the charge in coulombs (C), I is the current in amperes (A), and t is the time in seconds (s).

To find the electricity consumption, we need to calculate the charge passed through the electrolyte and convert it to the number of moles of electrons (n) using Faraday's constant (F): n = Q / F where F is the Faraday constant (96,485 C/mol).

Since we know the decrease in mass of the silver anode (5.4 g), we can calculate the number of moles of silver (Ag) dissolved using its molar mass (107.87 g/mol): moles of Ag = mass of Ag / molar mass of Ag

Finally, we can determine the electricity consumption by multiplying the number of moles of electrons (n) by the Faraday constant (F): electricity consumption = n * F

Please provide the current (I) and time (t) values used during the electrolysis process so that we can calculate the electricity consumption accurately.