How hydroxide primary batteries carry out spontaneous redox reactions

H2 has strong reducibility, O2 oxidation is stronger, in contrast, O2 has a strong effect on electrons, and H2 is more likely to lose electrons, so when hydrogen and oxygen are introduced, hydrogen is decomposed into hydrogen ions H+ and electrons E- at the negative electrode, electrons E- will flow along the wire to the positive electrode, (electrons will not enter the electrolyte solution), hydrogen ions will enter the electrolyte solution (the electrolyte you give is Koh, and the hydrogen ions will quickly react with hydroxide to form water), and on the positive electrode, the oxygen electrons are reduced (O2 + occurs under alkaline conditions 2H2O + 4E == 4OH ), it is important to note here that different electrolyte solutions will affect the form of the electrode reaction products, and of course the total reaction formula is fixed.

In addition, the reason for not igniting is that the oxygen that occurs under ignition conditions is too violent, and the hydrogen will lose electrons to give oxygen without ignition, and it seems that the battery is not heated either.

Feel free to ask!

First of all, it should be clear that the galvanic cell reaction is to disassemble a redox reaction and divide it into two stages, not necessarily the reaction between the electrode and the electrolyte solution, the electrolyte solution in the galvanic cell is likely to only play a role in enhancing conductivity, hydrogen is a strong reducing gas, oxygen is a very oxidizing gas, according to the redox reaction mantra "the reducing agent is reducing, the oxidation reaction occurs, the valency increases, the electrons are lost, the oxidant is oxidizing, the reduction reaction occurs, the valency decreases, and the electrons are obtained". The negative electrode hydrogen loses electrons and becomes hydrogen ions, which combine with hydroxide in an alkaline environment to form water, and the positive oxygen electrons become negative divalent oxygen ions, and combine with water to form hydroxide, in this reaction, electrons flow from the negative electrode to the positive electrode, and the direction of the current we define is the opposite direction of the directional movement of electrons (electrons are negatively charged) It should be noted that in the galvanic cell reaction, the electrolyte solution is always electrically neutral, so the electrons do not enter the solution.

One of the conditions for the formation of galvanic cells is to have a spontaneous redox reaction because this reaction can produce an electric current.

In telecom early pools, both the positive and negative electrodes are made of specific materials that can undergo redox reactions during the battery's overworking run. In a redox reaction, the material of the positive electrode is oxidized, while the material of the negative electrode is reduced. These two reactions are opposed to each other, i.e., when the material of the positive electrode is oxidized, the material of the negative electrode is reduced and vice versa.

When the battery is working, there is a reaction between the cathode material and the solution, and at the same time, there is a reaction between the anode material and the solution. These two reactions are antithetical to each other, so when the cathode material is oxidized, the anode material is reduced and vice versa. In this way, an electric current is generated that allows the battery to be powered.

Therefore, the reaction between the positive and negative electrodes of the battery is a spontaneous redox reaction, which is why one of the conditions for the formation of galvanic batteries is to be a spontaneous redox reaction.

I don't know if this explanation is correct, please correct.

The electrolysis of water to produce hydrogen and oxygen is a reduction and oxidation reaction, but not a redox reaction in the traditional sense. This is because redox reactions require the transfer of electrons, but during the hydrolysis process, electrons are not transferred from one atom or molecule to another.

Water molecules are electrolyzed into oxygen and hydrogen in an electrochemical electrolysis reaction, which is an electrolysis reaction rather than a redox reaction. When water molecules are electrolyzed, they are broken down into oxygen and hydrogen ions, and electrons are transferred directly to the electrodes rather than to their successors.

Therefore, although the water splitting reaction contains the reaction of reduction and oxidation of Qingshu, it is not a typical redox reaction, but an electrolytic reaction.

In all electrolytic reactions, an electric current passes through an electrolyte solution, and a redox reaction occurs on the cathode of the anode and the cathode. All electrolysis reactions are redox reactions, and the conversion of water electrolysis into hydrogen and oxygen is no exception, which belongs to redox reactions.

Answer: The generation of hydrogen and oxygen by water electrolysis is a redox reaction, water is both an oxidant and a reducing agent, hydrogen is a reduction product, and oxygen is an oxidation product.

Any redox reaction that takes place spontaneously can be designed as a galvanic cell because a galvanic cell is a type of battery with a spontaneous electric potential that works on the principle of redox reaction. Galvanic cells have a controllable electric potential that converts spontaneous redox reactions into a controllable electric potential, enabling the conversion and storage of electricity.

The structure of the galvanic cell is composed of a positive electrode, a negative electrode and an electrolytic destructive substance, wherein the positive electrode and the negative electrode are the catalysts for the redox reaction respectively, and the electrolyte plays the role of transferring electrons, when the positive electrode and the negative electrode are connected to the power supply respectively, the positive electrode undergoes oxidation reaction, and the negative electrode undergoes a reduction reaction, because the redox reaction can produce electric potential, so the galvanic battery can convert the spontaneous redox reaction into a controllable electric potential, so as to realize the conversion and storage of electricity.

Redox reactionsIt is a chemical base reaction, which involves the oxidation and reduction of substances. In redox reactions, some substances change from a low oxidation state to a high oxidation state, while others change from a high oxidation state to a low oxidation state. This reaction is characterized by the fact that the oxidizing agent separates the oxygen atom from another substance, while the reducing agent binds the oxygen atom to another substance.

For example, redox reactions can be used to treat contaminants in water. In this reaction, oxidizing agents such as oxygen and oxidants oxidize the contaminants, while reducing agents such as sodium carbonate separate the oxygen atoms from the contaminants, making them safer.

Galvanic batteries are designed on the principle of using chemical reactions to produce electrical energy, which includes electrodes and electrolytes inside the battery. The electrodes are the two parts of the battery that have a voltage difference between them, and when an electric current passes through the battery, the electrolyte undergoes a chemical reaction to produce electrical energy. The electrolyte consists of a positive electrode material and a negative electrode material, and the reaction between them produces electrons, which in turn produce electrical energy.

Answer]: The reason for the error is that many reactions in the potato hole in the galvanic battery are not redox reactions, such as concentration difference batteries, acid-base reaction batteries, ionization and sinking of insoluble electrolytes and ligands, and weak acid-base dissociation batteries.

In the spontaneous reaction, the outside of the anode material is full of outermost free-moving electrons e-, due to the attraction of anion and ion, the positively charged ions in the electrolyte solution are attached to the outside, and the more negative electrode materials react, the more negative ions are arranged outside, and the reaction is difficult to carry out (electron gain and loss: difficult). In galvanic cells, electrons are transferred from the negative electrode material to the positive electrode material, the positron in the electrolyte solution is reduced to obtain electrons, and the negative electrode material is oxidized and electrons are lost, and the reaction is very easy to carry out (electron gain and loss are easy).

Let's give you an example. For example, the reaction between zinc and sulfuric acid and the zinc-copper galvanic battery, when zinc reacts with sulfuric acid, zinc is responsible for losing electrons and reducing hydrogen ions on it, just like the kind of bus with only one door, people who get on and off the bus can only go through that door, so the rate is slow. In the reaction of zinc-copper galvanic batteries, zinc is only responsible for losing electrons, and hydrogen ions are reduced on copper, just like a bus in the city with two doors, the front and back doors are down, and the rate is naturally faster.

The same is true for other reactions.

Because only redox reactions have the gain and loss of electrons and the change of position.

Non-redox battery symbols can only be written in the attempt method.

The premise is that you need to be very familiar with the basic type of electric sideshow.

First, it is split into 2 electrode reactions (you don't have to worry about the positive and negative electrodes, you can specify the positive and negative electrodes arbitrarily) ag - e ag+

ag - e- +cl- →agcl

Then write the corresponding battery symbol, ag(s)|ag+(c1)agcl(s),ag(s)|cl-(c2) arbitrarily specifies an electrode as the negative pole and writes the battery symbol, for example.

agcl(s),ag(s)|cl-(c2) |ag+(c1)|ag(s)（+

Write out the electrode reactions for your specified battery and add them together to get the total reactions. Note that at this time, the positive and negative electrodes have been specified.

ag - e → ag+

agcl + e- →ag + cl-

agcl = ag+ +cl-

It was found that the total reaction was exactly the opposite of the response given by the question, so the positive and negative poles of the specified battery were reversed, and the correct battery (-)ag(s)|ag+(c1) |cl-(c2)|agcl(s),ag(s)（+

Hydrogen and oxygen in sodium hydroxide solution form the electrode reaction formula of the galvanic battery.

Positive electrode: O2 + 4E + 2H2O = 4Oh-

Negative electrode: 2h2-4e+4oh-

4h2o