Respuesta :
The reaction in which Cl has been oxidized is [tex]\rm Br_2\;+\;2\;Cl^-\;\rightarrow\;Cl_2\;+\;2\;Br^-[/tex]. Thus, option A is correct.
In a reaction, the oxidation has been defined as the loss of electrons by the atom, while reduction has been depicted as the gain of electrons.
The loss of electrons imparts a positive charge to the atom, while the gain of electrons imparts a negative charge to the atom.
In the following reactions, the Cl has been given as:
- [tex]\rm Br_2\;+\;2\;Cl^-\;\rightarrow\;Cl_2\;+\;2\;Br^-[/tex]
The chlorine has loses the electron and is converted to diatomic molecule. Thus, the Cl has been oxidized. The oxidation state of Cl has also been increased from -1 to 0.
- [tex]\rm Cl_2\;+\;2\;e^-\;\rightarrow\;2\;Cl^-[/tex]
The chlorine gains 2 electrons in the reaction and has been reduced.
- [tex]\rm 2\;ClO_3^-\;+\;12\;H^+\;\rightarrow\;Cl_2\;+6\;H_2O[/tex]
There has been no change in the oxidation state of chlorine. Thus, Cl has not been oxidized.
- [tex]\rm 2\;Na\;+\;Cl_2\;\rightarrow\;2\;NaCl[/tex]
The chlorine gains electron and has been converted to the Cl ion. With the gain of electrons, Cl has been reduced.
The reaction in which Cl has been oxidized is [tex]\rm Br_2\;+\;2\;Cl^-\;\rightarrow\;Cl_2\;+\;2\;Br^-[/tex]. Thus, option A is correct.
For more information about oxidation, refer to the link:
https://brainly.com/question/11507294
