Question #b2056

2 Answers
David Drayer
Apr 8, 2017

The Chlorine is the oxidizing agent. The Bromine is the reducing agent.

Explanation:

#2 Na^+Br^-1 + Cl_2^o = 2 Na^+Cl^- + Br_2^o#

Cl goes from a zero charge to a -1 charge The chlorine has been reduced its charge has gone down.

Br goes from -1 to a zero charge. The Bromine has been oxidized it charge has gone up

anor277
Apr 8, 2017

#NaBr(s) + 1/2Cl_2(g) rarr NaCl(s) + 1/2Br_2(l)#, and this is a stoichiometrically balanced equation.

Explanation:

And if we assign oxidation numbers, we can immediately see the direction of electron transfer:

#stackrel(+I)(Na)stackrel(-I)(Br)(s) + 1/2stackrel(0)Cl_2(g) rarr stackrel(+I)(Na)stackrel(-I)(Cl)(s) + 1/2stackrel(0)Br_2#

Bromide ion has been oxidized; chlorine gas has been reduced. Note (i) that you simply must know that the halogens are normally bimolecular; we represent them as #X_2#.

Also note (ii) that we probably could not get this reaction to work, even if thermodynamics is on our side.

Related questions
See all questions in Oxidation and Reduction Reactions
Impact of this question
1704 views around the world
You can reuse this answer
Creative Commons License