Chemistry, 28.10.2019 02:31 xolocsin

What happens to a reducing agent during a redox reaction?
the reducing agent is reduced.

the reducing agent is oxidized.

the reducing agent remains unchanged.

the reducing agent gains electrons.
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Answer from: Blackhawk1881

The reducing agent is oxidized during a redox reaction

$\boxed{\boxed{\bold{Further~explanation}}}$

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:

1. Binding/release of oxygen

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

2. Electron release / binding reaction

Oxidation is an electron release event

Example:

2F ---> 2Fe³⁺ + 6e⁻

The reduction is an electron capture event

Example:

3O₂ + 6e⁻ ---> 3O²⁻

3. The reaction of addition/reduction of oxidation number

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

In this reaction, it is also known

Reducing agents are substances that experience oxidation

The oxidizer is a substance that is reduced

Let's look at the answer choices

The reducing agent is reduced.

This statement is wrong because the reducing agent undergoes oxidation

The reducing agent is oxidized.

This statement is true

The reducing agent remains unchanged.

The statement is wrong because the oxidation number of the oxidized compound will increase

The reducing agent gains electrons.

The statement is wrong because the reducing agent releases electrons

So the correct statement is B The reducing agent is oxidized

$\boxed{\boxed{\bold{Learn~more}}}$

chemical reactions are an oxidation-reduction reaction

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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

What happens to a reducing agent during a redox reaction? the reducing agent is reduced. the reduci

Answer from: Quest

thats a little if u want the answer just look it up on google thats what i do haha : )

Draw the orbitals for the elements and give their number of electrons

Answer from: Quest

Answerthis solution will not form a precipitateexplanationsolubility equilbrium: pbf₂(s) ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is $k_{sp} = [\text{pb}^{2+}][\text{f}^- ]^2 = 4 \times 10^{-8}$ (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as $q = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}}$ then, we can interpret q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product: $\begin{aligned} q & = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}} \\ & = (1.9 \times 10^{-3} ) (3.8\times 10^{3})^2 \\ & = 2.7 \times 10^{-8} \end{aligned}$ since q = 2.7 × 10⁻⁸ < ksp = 4 × 10⁻⁸, a precipitate will not form.

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What happens to a reducing agent during a redox reaction?
the reducing agent is reduced.

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