Respuesta :
The given net reaction is:
Tl³⁺(aq) + 2Cr²⁺ (aq) → Tl⁺(aq) + 2Cr³⁺(aq)
The half cell reaction are:
Anode(Oxidation): Involves loss of electrons
Cr²⁺(aq) ↔ Cr³⁺(aq) + e⁻ ----------(1)
Cathode(reduction) : Involves gain of electrons
Tl³⁺ (aq) + 2e⁻ ↔ Tl⁺ (aq) ---------(2)
The net equation can be obtained by: 2* eq(1) + eq(2)
Cr²⁺(aq) ↔ Cr³⁺(aq) + e⁻ ----------(1)*2
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2Cr²⁺(aq) ↔ 2Cr³⁺(aq) + 2e⁻
Tl³⁺ (aq) + 2e⁻ ↔ Tl⁺ (aq) --
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Tl³⁺(aq) + 2Cr²⁺ (aq) → Tl⁺(aq) + 2Cr³⁺(aq)
The study of the chemical in the cell is called electrochemistry.
The correct answer is mentioned below.
What is standard cell potential?
- In electrochemistry, the standard electrode potential is defined as "The value of the standard emf of a cell in which molecular hydrogen under standard pressure is oxidized to solvated protons at the left-hand electrode".
The given net reaction is given as follows:-
[tex]Tl^{3+}(aq) + 2Cr^{2+} (aq) -----> Tl^+(aq) + 2Cr^{3+}(aq) [/tex]
The half cell reaction is: Anode(Oxidation): Involves loss of electrons
- [tex]Cr^{2+}(aq) <----> Cr^{3+}(aq) + e^- [/tex]
Cathode(reduction) : Involves gain of electrons
- [tex]Tl^{3+} (aq) + 2e^- <---> Tl^+ (aq) [/tex]
Hence, the two-cell reaction is described as mentioned.
For more information about the galvanic cell, refer to the link:-
https://brainly.com/question/6587304
