Question

Balance the following oxidation-reduction reactions, which take place in acidic solution, by using the "half-reaction" method.
a. Mg(s) + Hg2+(aq) -> Mg2+(aq) + Hg2(2+)(aq)

Answer 1

First, split the reaction up into the 2 half-reactions.

Answer 2

okay, i got that part done i just don't get the part where I have to add 2e- to the Hgs

Answer 3

since the Mg goes from Mg --> Mg+2, it has to lose 2 electrons to do that. Those electrons have to go somewhere, so the only other place is to give them to the Hg+2 ions

Answer 4

is this right..?
Mg(s) -> Mg2+(aq) 4Hg2+(aq) ->2Hg2(2+)(aq)
+2e- +2e-

Answer 5

you ahve to balance each lhalf reaction separately first, then add them back together at the end.

Answer 6

\[Mg \rightarrow Mg^{+2} + 2e^{-1}\]and\[2Hg^{+2} +2e^{-1} \rightarrow Hg_2^{+2}\]

Answer 7

ohh i thought i would multiply 2Hg+2 by 2 again haha :)

Answer 8

Mg(s) +2Hg2+(aq) -> Mg2+(aq) + 2Hg2(2+)(aq)? :3?

Answer 9

I also need help with this one please :)
NO3-(aq) + Br-(aq) -> NO(g) + Br2(l)

Answer 10

How would i balanced nitrogen and oxygen
NO3-(aq) -> NO(g)...?