Respuesta :
Answer: Order of the species in their decreasing oxidizing agent ability is [tex]Ag^+>Sn^{2+}>Cr^{3+}>Na^+[/tex]
Explanation: Oxidizing agent is defined as the agent which helps the other element to get oxidized and it itself gets reduced. These agents should have a positive value of reduction potentials. More is the positive value, best is the oxidizing agent.
Reducing agents are defined as the agents which helps the other element to get reduced and itself gets oxidized. These agents have a negative value of reduction potentials. The more the negative value, best is the reducing agent.
Reduction potentials of the following elements are:
[tex]Ag^+:0.80V\\Cr^{3+}:-0.74V\\Sn^{2+}:-0.14V\\Na^+:-2.71V[/tex]
From the given reduction potentials, the best oxidizing agent is [tex]Ag^+[/tex] and the best reducing agent is [tex]Na^+[/tex]
Order in the decreasing oxidizing agent ability of the species is [tex]Ag^+>Sn^{2+}>Cr^{3+}>Na^+[/tex]
From best oxidizing agent to best reducing agent : Ag⁺, Sn²⁺, Cr³⁺, Na⁺
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 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
Oxidizing agents are substances that experience reduction
The metal activity series is expressed in voltaic series
Li-K-Ba-Ca-Na-Mg-Al-Mn- (H2O) -Zn-Cr-Fe-Cd-Co-Ni-Sn-Pb- (H) -Cu-Hg-Ag-Pt-Au
The more to the left, the metal is more reactive (easily release electrons) and the stronger reducing agent
The more to the right, the metal is less reactive (harder to release electrons) and the stronger oxidizing agent
So that the metal located on the left can push the metal on the right in the redox reaction
From the ion ion below:
Ag⁺ ;Cr³⁺ ;Sn²⁺; Na⁺
If we sort according to the voltaic series: (from left to right)
Na, Cr, Sn, Ag
Then:
Na, the most reactive, strong reducing agent
Ag, less reactive, strong oxidizing agents
So that the order from best oxidizing agent to best reducing agent.
Ag⁺, Sn²⁺, Cr³⁺, Na⁺
Learn more
an oxidation-reduction reaction
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a reducing agent during a redox reaction
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loses electrons in a chemical reaction
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Keywords: reduction, oxidation
