Which of the following chemical reactions is an oxidation-reduction reaction? (3 points) question 4 options: 1) cuso4 + bacl2 yields baso4 + cucl2 2) pb(no3)2 + 2nacl yields pbcl2 + 2nano3 3) n2 + 3h2 yields 2nh3 4) k2so4 + bacl2 yields baso4 + 2kcl

Given are:

1) CuSO4 + BaCl2 ---> BaSO4 + CuCl2
2) Pb(NO3)2 + 2NaCl ---> PbCl2 + 2NaNO3
3) N2 + 3H2---> 2NH3
4)K2SO4 + BaCl2---> BaSO4 + 2KCl

Among the 4 reactions above, the only oxidation - reduction reaction is number 3:

N2 + 3H2 > 2NH3 

since the oxidation numbers of N and H decreased and increased, respectively making the reaction RedOx.  

The reaction including the redox reaction is reaction number 3

N₂ + 3H₂ ---> 2NH₃

There are elements that experience changes in oxidation number in the reaction

Oxidation is an increase in oxidation number, while reduction is a reduction in oxidation number.

The formula for determining Oxidation Numbers in general:

1. Single element atomic oxidation number = 0. Examples of Ar, Mg, Cu, Fe, N₂, O₂, etc. = 0

Group IA (Li, Na, K, Rb, Cs, and Fr): +1

Group IIA (Be, Mg, Ca, Sr and Ba): +2

H in compound = +1, except metal hydride compounds (Hydrogen which binds to groups IA or IIA) oxidation number H = -1, for example, LiH, MgH₂, etc.

2. Oxidation number O in compound = -2, except OF2 = + 2 and in peroxide (Na₂O₂, BaO₂) = -1 and superoxide, for example KO₂ = -1/2. 3 The oxidation number in an uncharged compound = 0,

Total oxidation number in ion = ion charge, Example NO₃⁻ = -1

In a redox reaction, it is also known

Reducing agents are substances that experience oxidation

An oxidizer is a substance that is reduced

Redox reactions are reactions that are accompanied by changes in oxidation number, so what must be examined is whether there are elements that experience changes in oxidation number in the reaction

1. CuSO₄ + BaCl₂ ---> BaSO₄ + CuCl₂

The oxidation number in this reaction, the elements having oxidation numbers remain good at reactants and products

Cu = + 2

SO₄ = -2

Ba = +2

Cl = -1

2. Pb (NO₃)₂ + 2NaCl ---> PbCl₂ + 2NaNO₃

The oxidation number of the elements involved is also constant

Pb = +2

NO3 = -1

Na = +1

Cl = -1

3. N₂ + 3H₂ ---> 2NH₃

In this reaction, there is a change in the oxidation number of elements N and H

N = from 0 to -3

H = from 0 to +1

N₂ undergoes a reduction reaction because the oxidation number drops while H₂ undergoes an oxidation reaction because the oxidation number rises

4. K₂SO₄ + BaCl₂ ---> BaSO₄ + 2KCl

The oxidation number of the elements involved is also constant

K = +1

SO₄ = -2

Ba = +2

Cl = -1

So that the reaction including the redox reaction is reaction number 3

N₂ + 3H₂ ---> 2NH₃

the reduction process

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an element's oxidation

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an element's oxidation number increase

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Keywords: oxidation, reduction, The oxidation number

The answer for this is a

Ionic compounds dissociate into component ions dissolved into a solution creating substances called "electrolytes".hope my answer has you : )