While investigating the chemical and physical properties of metallic element E, a student conducts an experiment by combining E(s) and HBr(aq), which react according to the following equation:
2E(s) + 2HBr(aq)----> 2EBr(aq)+H2(g)
a)write the net-ionic equation for the reaction.
b)in the reaction, is E(s) being oxidized or reduced? Justify your answer in terms of oxidation numbers.

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tutorareej tutorareej · Answer 1 · 2021-10-15T11:28:45+02:00

The net ionic equation for the reaction will be :

[tex]\rm 2\;H^+\;+\;2\;E^+\;+\;2Br^-\;\rightarrow\;H_2\;+2\;EBr[/tex]

In this reaction, E is being oxidized.

The ionic reaction can be written by the gain and loss of electrons and the formation of the product.

The ionic reaction can be divided into oxidization and reduction reaction:

[tex]\rm 2\;H^+\;+\;E\;(s)\;\rightarrow\;2\;E^+\;+\;H_2[/tex] ...... Oxidation reaction

[tex]\rm 2\;E^+\;+\;2\;Br^-\;\rightarrow\;2\;EBr[/tex] ...... Reduction reaction

With the gain of Hydrogen ions, the E is getting oxidized and Br is getting reduced in the reaction.

The net ionic equation will be :

[tex]\rm 2\;H^+\;+\;2\;E^+\;+\;2Br^-\;\rightarrow\;H_2\;+2\;EBr[/tex]

The element E is getting oxidized due to the gain of hydrogen ions in the reaction.

For more information about the oxidation and net ionic reaction, refer the link:

https://brainly.com/question/21883718?referrer=searchResults