Question

write the four effects of chemical reaction​

Answer 1

Answer:

1. physical state of the reactants and surface area.

2.Temperature.

3.presence of Catalyst.

4. Reactant concentration.

Answer 2

Explanation:

FOUR BASIC TYPES :

Synthesis:

In a synthesis reaction, two or more simple substances combine to form a more complex substance. These reactions are in the general form:

{\displaystyle {\ce {A + B -> AB}}}

Two or more reactants yielding one product is another way to identify a synthesis reaction. One example of a synthesis reaction is the combination of iron and sulfur to form iron(II) sulfide:

{\displaystyle {\ce {8Fe + S8 -> 8FeS}

DECOMPOSITION:

Decomposition reaction is when a more complex substance breaks down into its more simple parts. It is thus the opposite of a synthesis reaction, and can be written as[18][1]

{\displaystyle {\ce {AB -> A + B}}}

One example of a decomposition reaction is the electrolysis of water to make oxygen and hydrogen gas:

{\displaystyle {\ce {2H2O -> 2H2 + O2}}}

Single replacement

In a single replacement reaction, a single uncombined element replaces another in a compound; in other words, one element trades places with another element in a compound[18] These reactions come in the general form of

{\displaystyle {\ce {A + BC -> AC + B}}}

One example of a single displacement reaction is when magnesium replaces hydrogen in water to make magnesium hydroxide and hydrogen gas:

{\displaystyle {\ce {Mg + 2H2O -> Mg(OH)2 + H2 (^)

Double replacement

In a double replacement reaction, the anions and cations of two compounds switch places and form two entirely different compounds.[18]These reactions are in the general form:[19]

{\displaystyle {\ce {AB + CD -> AD + CB}}}

For example, when barium chloride (BaCl2) and magnesium sulfate (MgSO4) react, the SO42− anion switches places with the 2Cl−anion, giving the compounds BaSO4 and MgCl2.

Another example of a double displacement reaction is the reaction of lead(II) nitrate with potassium iodide to form lead(II) iodide and potassium nitrate:

{\displaystyle {\ce {Pb(NO3)2 + 2KI -> PbI2(v) + 2KNO3}

Oxidation and reduction:

Redox reactions can be understood in terms of transfer of electrons from one involved species (reducing agent) to another (oxidizing agent). In this process, the former species is oxidized and the latter is reduced. Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always change the oxidation state, but there are many reactions that are classed as "redox" even though no electron transfer occurs (such as those involving covalent bonds).[20][21]

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MARK AS BRAINLEAST ANSWER