Question

Question #b2056

Answer 1

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

Answer 2

`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.