oxidizing agent?

Question

A colorless solution of KBr is added to a colorless solution containing Cl_2.

What's the balanced net ionic eq (no spectator ions) for this, assuming the rxn occurs? And what's the oxidizing agent? thanks again.

Answer 1

Lancenigo di Villorba (TV), Italy

QUESTION a)
2 Br-(aq) + Cl2(aq) ---> 2 Cl-(aq) + Br2(l)
In effect, another reaction may run.

QUESTION b)
Chlorine is the OXIDIZER.

ABOUT THIS EXPERIMENT
If you add some "Chlorine's water" 's drops to an aqueous solution of KBr, you may note a yellowish coloration.
I may refer to the following reaction :

2 KBr(aq) + Cl2(aq) ---> 2 KCl(aq) + Br2(l)

where bromine gives a PALE COLORATION to this solution instead pure bromine shows a reddish hue. In effect, water is not the best solvents for bromine, hence you must repeat this experiment adding some drops of carbon tetrachloride even : bromine appears in its reddish coloration.
On the other hand, if you force the chemical system adding furtherly "chlorine's water", the reddish hue disappears

Br2(l) + Cl2(aq) ---> 2 BrCl(l)

I highlight that "(aq)" means "in aqueous phase" while "(l)" means "in another liquid phase".
Among the different chemical stuffs involved, only bromine is coloured (red).

I hope this helps you.

Answer 2

since the oxidation no. of Br reduces from -1 to 0, it is oxidised. so, Br is definitely the oxidising agent.

Answer 3

2KBr + Cl2 -> 2KCl + Br2

2K+ + 2Br- + Cl2 -> 2K+ + 2Cl- + Br2


net ionic : 2 Br- + Cl2 -> 2Cl- + Br2


oxidizing agent : bromide ..


( not sure though.. :P)

Answer 4

maybe bromine?