You are studying the reaction A2(g) + B2(g) →→ 2AB(8)
to determine its rate law. Assuming that
you
have a valid exper-
imental procedure for obtaining [A2] and [B2] at various times,
explain how you determine (a) the initial rate, (b) the reaction
orders, and (c) the rate constant.

The Mg element is the reducing agent and the Fe element is the oxidizing agent

The oxidation-reduction reaction or abbreviated as Redox is a chemical reaction in which there is a change in oxidation number

3 basic theories explain this Redox concept:

The oxidation reaction is the binding of a substance with oxygen. (O₂)

For example:

2SO₂ + O₂ ----> 2SO₃

The reduction reaction is the release of oxygen from a substance.

For example:

2CuO → 2Cu + O₂

Oxidation is an electron release event

Example:

2F ---> 2Fe³⁺ + 6e⁻

The reduction is an electron capture event

Example:

3O₂ + 6e⁻ ---> 3O²⁻

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

In the redox reaction, it is also known

Reducing agents are substances that experience oxidation

The oxidizing agent is a substance that is reduced

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 IA or IIA groups) 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

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

Let's look at the reaction

Mg(s)+Fe²⁺(aq)→Mg²⁺(aq)+Fe(s)

Let see the change in the oxidation number of each element

Mg on the left = 0 (single element)

Fe²⁺ on the left = +2 ( ion charge)

Mg on the right = +2 ( ion charge)

Fe on the right = 0 (single element)

Means that the element Mg has increased oxidation number from 0 to +2 so that it experiences an oxidation reaction and acts as a reducing agent

While Fe has decreased the oxidation number from +2 to 0, so it has a reduction reaction and acts as an oxidizer

an oxidation-reduction reaction

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a reducing agent

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element is reduced

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Keywords: oxidation-reduction, an oxidizing agent, a reducing agent