Find 20 Redox Reaction Formula
1. $2Mg + O_{2}\stackrel{点燃}{=\!=\!=}2MgO$ 2. $3Fe + 2O_{2}\stackrel{点燃}{=\!=\!=}Fe_{3}O_{4}$ 3. $2Cu + O_{2}\stackrel{\Delta}{=\!=\!=}2CuO$ 4. $F_{2} + H_{2} =\!=\!= 2HF$ 5. $F_{2} +Xe(过量)=\!=\!=XeF_{2}$ 6. $2F_{2}(过量)+Xe=\!=\!=XeF_{4}$ 7. $nF_{2} +2M=\!=\!=2MF_{n}$（表示大部分金属） 8. $2F_{2} +2H_{2}O=\!=\!=4HF+O_{2}$ 9. $2F_{2} +2NaOH=\!=\!=2NaF+OF_{2} +H_{2}O$ 10. $F_{2} +2NaCl=\!=\!=2NaF+Cl_{2}$ 11. $F_{2} +2NaBr=\!=\!=2NaF+Br_{2}$ 12. $F_{2}+2NaI =\!=\!=2NaF+I_{2}$ 13. $F_{2} +Cl_{2} (等体积)=\!=\!=2ClF$ 14. $3F_{2} (过量)+Cl_{2}=\!=\!=2ClF_{3}$ 15. $7F_{2}(过量)+I_{2} =\!=\!=2IF_{7}$ 16. $Cl_{2} +H_{2} =\!=\!=2HCl$ 17. $3Cl_{2} +2P=\!=\!=2PCl_{3}$ 18. $Cl_{2} +PCl_{3} =\!=\!=PCl_{5}$ 19. $Cl_{2} +2Na=\!=\!=2NaCl$ 20. $3Cl_{2} +2Fe=\!=\!=2FeCl_{3}$ 点击前往免费阅读更多精彩小说
Handwritten notes on the Redox Reaction
The following is an example of a handwritten note on a reduction reaction: * * 1. Basic Concepts ** 1. * * Reaction Type ** - Oxidation reaction: A reaction in which the chemical valency of the elements contained in a substance increases. - Reductive reaction: A reaction in which the chemical valency of the elements contained in a substance is reduced. - Oxidation-reduction reaction: There are reactions where the valency of elements increases and decreases. 2. * * Reactants ** - Oxidant: A substance that obtains electrons in a reaction. - Reductant: A substance that loses electrons during a reaction. 3. * * Production ** - [Oxidation product: The product obtained after the loss of electrons.] - [Reductive product: The product obtained after electrons are reduced.] 4. * * Material Nature ** - Oxidability: The property of the electron emitted by the initiator. - Reductibility: The property of a reducing agent that loses electrons. * * 2. Common Oxidants and Reductants ** 1. * * Judgment basis (mainly depends on the element's valency)** - When the element is at the highest valency, the element can only be used as an oxidiser, such as Mn with +7 valency and S with +6 valency. - When an element was in an intermediate state, it could act as both an oxidiser and a reducing agent, such as S with 0 valency and S with +4. - When an element is at its lowest price, it can only be used as a reducing agent, such as S with a-2 valency. 2. * * Important Oxidants ** - Active non-metallic elements, such as F2, Cl2, Br2, O2, etc. - When the element is at a high price, it is an oxide-containing acid, a high-priced ox-containing acid, and a high-priced ox-containing acid salt, such as MNO2, NO2; concentrated H2SO4, HNO3; KMNO4, KClO3, FeCl3, etc. - Peroxides, such as Na2O2, H2O2, etc. 3. * * An important reducing agent ** - Elemental metals such as Na, K, Mn, and Mn. - Some non-metallic elements, such as H2, C, Si, etc. - Oxides of elements with low valency, such as CO, SO2, etc. - An acid when the element is at a low valency, such as HQ (concentrated), Brr, Hi, H2S, etc. - The salt when the element is at a low valency, such as Na2SO3, FeSO4, etc. * * 3. Description of electron transfer ** 1. * * Double Line Bridge Method ** - The arrow points from the element in the reagent that has changed its valency to the same element in the product that has changed its valency (an arrow goes up and an arrow goes down, crossing the equal sign in the middle of the equation). - Number of electrons transferred: When the valency increases, electrons are lost; when the valency decreases, electrons are gained. The valency changes the number of atoms of the element m × the number of electrons gained (or lost) per atom ne-, which is m × ne-. 2. * * Single-line bridge method ** - The line bridge started from the element with a higher chemical valency in the reagent and pointed to the element with a lower chemical valency in the reagent. The arrow pointed to the element with a lower chemical valency in the initiator, and the arrow was just "=". - The total number of electrons transferred was indicated on the wire bridge, and neither gained nor lost was written. * * 4. Reaction Law of Oxidation-reduction Reaction ** 1. * * Price State Law ** - The same element, in its highest state, was only oxidiser. In the lowest state, it only has reduction. In the intermediate state, it has both oxidisation and reduction properties. 2. * * Dissimilation and Reincarnation Rule ** - The law of the return of the valency state: When the same element has different valency states, the change of the valency state is "only close to each other, can be intersected, and not crossed". 3. * * Reaction sequence ** - In a solution of similar concentration: - At the same time, when a concentrated reducing agent is added, the strong reducing agent will be first oxided. - At the same time, when it contains a concentrated oxidiser, after adding a reducing agent, the strong oxidiser will be reduced first. 4. * * Law of Conservation ** - In any oxido-reduction reaction, the total number of increase in valency = the total number of decrease in valency, the total number of electrons lost by the reducing agent = the total number of electrons obtained by the oxidiser, and the number of charges before and after the reaction was equal. * * 5. Rule of Judging the Strength of Oxidability and Reductibility ** 1. * * Judgement based on the equation of the oxido-reduction reaction ** - Oxidability: Oxidants> Oxidation products. - Reductibility: reducing agent> reducing product. It can be summed up as: what kind of agent to find, the nature of the product is weaker than the agent. 2. * * Judging by the metal activity sequence ** - The reduction of K, Na, Na, Mn, Al-Mn, Fe-Mn, Sn-P,(H), Cu-Mn, Ag-Mn, Pt-Mn gradually weakened from left to right, and the oxidisation of the corresponding ions gradually increased. 3. * * Based on reaction conditions and intensity ** - The lower the reaction conditions, the more intense the reaction, and the stronger the oxidisation or reduction of the corresponding substance. 4. * * Based on the degree of the oxido-reduction reaction ** - Under the same conditions: - When different oxidisers act on the same reducing agent, the higher the price of the oxidiser, the stronger the oxidiser. - Different reducing agents acted on the same kind of oxidiser, and the reduction product with a low valency had a strong reduction ability. * * 6. Balance of the Redox Reaction Formula ** 1. * * Three Principles ** - The principle of electron conservation, the principle of atom conservation, and the principle of charge conservation. 2. * * General Method ** - Valence rising and falling method combined with the least common multiple method. 3. * * Balance technique (balancing the missing equation of the oxido-reduction reaction)** - First, he used the "valency increase and decrease method" to balance the chemical quantities of substances with variable valency elements. Then, he used the conservation of atoms to determine the unknown, and then he balanced them according to the conservation of atoms. - The principle of complementing: - Under acidic conditions, if there was a lack of H (hydrogen) or more O (oxygen), H + would be supplemented. If there was less O (oxygen), H2O (water) would be supplemented. - Under basic conditions, if there was a lack of H (hydrogen) or more O (oxygen), H2O (water) would be supplemented, and if there was less O (oxygen), it would be supplemented with Oh-. The balancing order of the equations for the oxido-reduction reaction involving ions: - According to the rise and fall of the chemical valency, the chemical quantities of the oxidiser, and the oxidiser were balanced. - According to the conservation of charge, the number of ions was adjusted. - Finally, he checked the conservation of atoms and charge. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Redox reaction advanced language
Oxidation-reduction reactions were a type of chemical reaction that was widespread in nature and had important significance in industrial production. In essence, the substances involved in the reaction had electron transfer or deviation before and after the reaction. This reaction was composed of an half-reaction of an oxidization and a half-reaction of a reduction. In the process of the reaction, the process of the element losing electrons and increasing the number of electrons was called an oxidization reaction; the process of the element gaining electrons and decreasing the number of electrons was called a reduction reaction. Redox reaction was first proposed by the French mathematician Lavoisier in 1774. It covered many types, including the reactions of minerals (such as metal corrosion, disproportionate reactions, etc.), electrochemistry, organic, biological, and geological reactions in soil. The reaction rate was affected by many factors such as the concentration of the reagents, the concentration of the acid, the temperature, the catalyst, and so on. The process of partial oxidoreduction reactions was more complicated. It was involved in many fields, such as the extraction, electrolysation, and plating of metals in the industrial field, the change of soil and fertilizer in the agricultural field, the burning of natural gas, oil, coal, and other fuel in the fossil energy field, the reaction of hydrogen and oxygen in new energy fuel cells, and the development of drugs and pharmacology. In addition, the self-developed electromagnetic light wave cold plasma advanced oxido-reduction reaction technology for waste permeate membrane concentrate is an advanced technology that combines electromagnetics, optical, plasma physics and the principles of chemical stabilization. Through the cooperative effects of electromagnetic light wave, cold plasma technology, and the introduction of oxidiser, it can deal with the hard-to-degrade organic matter and other impurities in the waste permeate membrane concentrate. It can realize the cycle process of organic molecular decomposition and decomposition. It has the characteristics of efficient decomposition. It was friendly to the environment and had a wide range of applications. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Redox Reaction of Metal Ions
The oxidoreduction reaction of metal ions included two aspects: reduction reaction and oxidization reaction. In the reduction reaction, the metal ions gain electrons, the number of electrons is reduced, and the metal ions change from a high to a low state, releasing electrons. For example, in some reaction systems, high-priced metal ions would become low-priced metal ions after obtaining electrons. In the oxidization reaction, the metal atom loses its electrons, and the oxidization number increases. It changes from a low-level state to a high-level state while absorbing electrons. The essence of this reaction was the transfer of electrons. In other words, metal atoms lost electrons and became metal ions (the oxidization process), and metal ions gained electrons and became metal atoms (the reduction process). The reaction was usually carried out in an acidic solution, and a reduction indicator was often used to observe the reaction process. In practical applications, the oxidoreduction reaction of metal ions was widely used in the fields of plating, metal corrosion and protection, metal extraction, and so on. Moreover, the metal ions 'oxido-reduction reaction followed the basic laws of electron conservation, charge conservation, and energy conservation. The mobility of a metal was also restricted by the ability of its ions to undergo reduction and oxidization reactions, which affected the properties and uses of the metal in chemical reactions. For example, the more mobile the metal was, the stronger the ability of its atoms to lose electrons, and the weaker the ability of its ions to gain electrons in the reduction reaction. The stronger the ability of its ions to lose electrons in the oxidization reaction, the weaker the ability of metal atoms to generate metal ions. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction Rate Formula
1. For a chemical reaction, the reaction rate was calculated as: <<v>=<cC>(g)>+<dD>(g)>(v =<Delta c>/<Delta t>)(<v>: average rate,<<Delta c>>: concentration change,<<Delta t>>: time), in units of </(L·s)>. 2. For elementary reactions, the expression of the mass action law can be used as the reaction rate equation, the reaction rate equation, r = k(A)^a(B)^b, where k is the specific reaction constant (a quantity independent of concentration). 3. For the reaction,<aA(g)+bB(g)=cC(g)>, the reaction rate <v_positive = k_positive c^a(A)·c^b(B)>,<v_inverse = k_inverse c^c(C)>, when the reaction reaches equilibrium,<v_positive = v_inverse>, that is,<k_positive c^a(A)·c^b(B)=k_inverse c^c(C)>. 4. When the same reaction was expressed by different substances, the values might be different, but the meaning was the same. The reaction rates expressed by different substances had the relationship of [v(A): v(B): v(C): v(D)=m: n: c: d](the ratio of the rates was equal to the ratio of the measurement factors of the corresponding substances). <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
First Order Reaction Formula of the Reaction Rate
The first-order reaction rate equation was: r = -dt/dt = kc, and its integral form was: Where, a is the concentration of the reagent at the beginning of the reaction, c is the concentration of the reagent at time t, and k is the rate constant. The unit is the negative power of the time unit, such as s^{-1}, min^{-1}, h^{-1}, d^{-1}, etc. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction Formula and Condition of the Reaction of the Acid and the Acid
Under normal circumstances, the reaction between the two could not be carried out directly. Because the lone pair of electrons of the oxygen of the alcoholic group was coupled with the aromatic ring, the reaction activity was very weak, and it could not be used to catalyze the ester reaction with the acid. To synthesize the ester, the reaction of an acid acid or an acid ether with the ether was usually done. For example, the reaction between the ether and the ether was: C6H50H +(CH3CO) 2O = CH3COOC6H5 + CH3COON. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction Formula for the Production of Water by Water Reaction
以下是几种水解制氢的反应式： 1. 铝水反应制氢： - \(2Al +4H_{2}O = 2AlO(OH)+3H_{2}\uparrow\) - \(2Al + 6H_{2}O=2Al(OH)_{3}+3H_{2}\uparrow\) 2. 硼氢化钠催化水解制氢：\(NaBH_{4}+2H_{2}O\stackrel{催化剂}{=\!=\!=}4H_{2}+NaBO_{2}\) <a href="/?from=ask_words" style="color:red" target="_blank">点击前往免费阅读更多精彩小说</a>
Reaction Formula of Substitution Reaction for the addition reaction of organic substances
Additional reaction: - The addition reaction of ethene and Bromine: <<CH2 = CH2 + Br2> - The addition reaction of ethene and hydrogen bromidate was as follows: <CH2 = CH2> - Under certain conditions, addition reactions could also occur between ethene, hydrogen, and water. Since the chemical properties of ethyne (carbon-carbon triple bond) were similar to that of alkene (carbon-carbon double bond), similar addition reactions could also occur. - The aromatic ring can undergo an addition reaction with hydrogen (in the presence of a catalyst such as Ni). - Aldol groups can undergo a reduction reaction (addition reaction), such as: <anno data-annotation-id ="00000000 - 4c00 - 4c00 - 8c00 - 9c00 - 9c000b000000"> CH3CH20H </anno>. Substitution reaction: - The substitution reaction between methane and Cl2: CH4 + Cl2. - The substitution reaction of the aromatic ring: For example, the substitution reaction with the aromatic group using FeBr3 as a catalyst; the nitration reaction with the aromatic group using concentrated sulfuric acid under heating conditions (the hydrogen on the aromatic ring is replaced by the nitrogen group). - The substitution reaction of the halated carbon was as follows: <<CH3CH2Br2>+<NaBr2>>. - The substitution reaction of alcohol: <CH3CH20H>+<br>> longrightarrow <CH3CH2br>+<H2O>> - The ester's cleavage reaction (which can be seen as a substitution reaction):<CH3COOCH2CH3 + H2O> <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction Formula of CaSO4 and CaCO3
The chemical equation of the reaction between calcium sulfuric acid (CaSO) and sulfuric acid (H ^CO) is: CaSO + H ^CO = CaCO + H ^SO. This was a metathesis reaction. During the reaction, the sulfuric acid ions (SO2) exchanged positions with the carbon dioxide ions (CO2) to form calcium carbonite and sulfuric acid. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction Formula of the Alkaline Cell
The reaction formula for the molten NaI is: $2NaI +2Na + I2 $, and the reaction formula for the molten NaI solution is: $2NaI +2H2O +2NaOx + I2 + H2 $. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>