Which of the following oxidizing agents will oxidize Br– but not Cl–? 2Br– ⇔ Br2(l) + 2e– E°ox = –1.065 V 2Cl– ⇔ Cl2(g) + 2e– E°ox = –1.359 V Cr2O72–(aq) + 14H+(aq) + 6e– T h i s a n s w e r i s s e t a s c o r r e c t 7H2O(l) + 2Cr3+(aq) E°red =+1.33 V MnO4–(aq) + 8H+(aq) + 5e– ⇔ Mn2+(aq) + 4H2O(l) E°red = +1.51V NO3–(aq) + 4H+(aq) + 3e– ⇔ NO(g) + 2H2O(l) E°red =+0.96 V

System having higher standard reduction potential than [tex]Br_{2}\mid Br^{-}[/tex] system but have lesser standard reduction potential than [tex]Cl_{2}\mid Cl^{-}[/tex] system will oxidize [tex]Br^{-}[/tex] but not [tex]Cl^{-}[/tex]

Higher reduction potential suggests higher tendency to consume electrons and lesser reduction potential suggest lower tendency to consume electrons or alternatively higher tendency to release electrons.

Therefore [tex]Cr_{2}O_{7}^{2-}\mid Cr^{3+}[/tex] system oxidizes [tex]Br^{-}[/tex] but not [tex]Cl^{-}[/tex].

shrutiagrawal1798 shrutiagrawal1798 · Answer 2 · 2022-03-21T08:44:32+01:00

Oxidation is defined as the loss of electrons, while reduction is the gain of electrons. The oxidizing agent for Br, but not for Cl is [tex]\rm Cr_2O_7^{2-}\;+\;14\;H^+\;+6\;e^-\;[/tex].

What is an oxidizing agent?

The oxidizing agent has been defined as the agent that gains the released electrons from the compound and reduces itself.

The oxidation potential has been the ability to lose the electron. The higher the oxidation potential, the higher ability to oxidize the compound with the lower potential.

The oxidation potential of Br is 1.065 V, and Cl is 1.359 V. Thus, the compound with oxidation potential greater than Br, and lesser than Cl, will oxidize Br, but not Cl.

The oxidation potential of chromium oxide is 1.33 V. Thus it will be able to reduce Br, but not Cl.

Learn more about the oxidizing agents, here;

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