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 oxidizes but not .

Explanation:

System having higher standard reduction potential than system but have lesser standard reduction potential than system will oxidize but not

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 system oxidizes but not .