Question

Привет!Очень нужна помощь!) Напишите уравнения реакций,происходящих на электродах и суммарные реакции при электролизе расплава и раствора соли MgCl2 с инертными электродами.Рассчитайте количество электричества необходимое для выделения на катоде 1 г-экв вещества при электролизе расплаве и раствора соли

Answer 1

Могу только уравнения реакций написать
При электролизе расплава :
На катионе:2Cl- -2е=Cl2
На анионе: Мg2+ +2е= Мg
Суммарное: МgCl2=Mg+Cl2
При элпктролизе раствора:
На катионе: 2Cl- -2е=Cl2
На анионе:2H2O+2e=2OH- +H2
Суммарное: 2Н2О+MgCl2=Cl2+Mg(OH)2+H2

Answer 2

Electrolysis of Molten and Aqueous MgCl2 with Inert Electrodes

Hey there! I'd be happy to help you with that. Let's start by writing the equations for the reactions occurring at the electrodes and the overall reactions for the electrolysis of molten and aqueous MgCl2 with inert electrodes.

Electrolysis of Molten MgCl2

The electrolysis of molten MgCl2 involves the decomposition of the compound into its constituent elements, magnesium and chlorine, at the respective electrodes.

At the Anode (Oxidation): The chloride ions (Cl-) are oxidized to chlorine gas (Cl2) and release electrons.

The half-reaction at the anode is: ``` 2Cl^- -> Cl2 + 2e^- ``` [[1 #1]]

At the Cathode (Reduction): The magnesium ions (Mg2+) are reduced to magnesium metal (Mg) by gaining electrons.

The half-reaction at the cathode is: ``` Mg2+ + 2e^- -> Mg ``` [[1 #1]]

Electrolysis of Aqueous MgCl2

In the case of the electrolysis of aqueous MgCl2, water also undergoes electrolysis along with the decomposition of MgCl2.

At the Anode (Oxidation): The water molecules are oxidized to oxygen gas (O2) and release protons (H+).

The half-reaction at the anode is: ``` 2H2O -> O2 + 4H+ + 4e^- ``` [[2 #2]]

At the Cathode (Reduction): The magnesium ions (Mg2+) are reduced to magnesium metal (Mg) by gaining electrons.

The half-reaction at the cathode is the same as in the case of the electrolysis of molten MgCl2: ``` Mg2+ + 2e^- -> Mg ``` [[1 #1]]

Overall Reactions

The overall reactions for the electrolysis of molten and aqueous MgCl2 with inert electrodes can be obtained by combining the half-reactions at the anode and cathode.

Molten MgCl2: The overall reaction for the electrolysis of molten MgCl2 is the combination of the anode and cathode half-reactions: ``` 2MgCl2 -> 2Mg + Cl2 ``` [[1 #1]]

Aqueous MgCl2: The overall reaction for the electrolysis of aqueous MgCl2 is the combination of the anode and cathode half-reactions, along with the electrolysis of water: ``` 2MgCl2 + 2H2O -> 2Mg + 2Cl2 + O2 + 4H+ ``` [[1 #1]] [[2 #2]]

Calculating the Amount of Electricity

To calculate the amount of electricity required to produce 1 gram-equivalent of substance during the electrolysis of molten and aqueous MgCl2, we can use Faraday's laws of electrolysis.

The amount of electricity required can be calculated using the formula: ``` Q = n * F ``` Where: - Q is the amount of electricity in coulombs (C) - n is the number of gram-equivalents of the substance - F is the Faraday constant (96,485 C/mol)

For 1 gram-equivalent of magnesium (Mg) produced: - n = 1 (since 1 gram-equivalent is being produced) - F = 96,485 C/mol

Substitute the values into the formula to calculate the amount of electricity required.

I hope this helps! Let me know if there's anything else you'd like to discuss.