Question

Balance the following oxidation-reduction reactions, which take place in acidic solution, by using the "half-reaction" method.
NO3-(aq) + Br-(aq) -> NO(g) + Br2(l)

Answer 1

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

Answer 2

what's an A-level i'm trying to balance equations on here..

Answer 3

\[(2Br^- \rightarrow Br_2+2e^-) \times 3\]
\[(3e^-+4H^++NO_3 \rightarrow NO+2H_2O)\times 2\]
-------------------------------------------------
\[6Br^- \rightarrow 3Br_2 +\cancel{6e^-}\]
\[\cancel{6e^-}+8H^++2NO_3 \rightarrow 2NO+4H_2O\]
--------------------------------------------------------

Answer 4

so would this be the correct answer..?
2NO3-(aq) + 8H+ +6Br-(aq) -> 2NO(g) + 4H2O + 3Br2(l)..? :P

Answer 5

i dont think it's right cause the equations don't balance
on the right side its 2+8+6=16
and on the left side its 2+4+3=9

Answer 6

You say the charges?
Left side is
-6+8-2=0

Right side has no charges, 0

Answer 7

no the elements

Answer 8

No, you don't balance element by adding them,
balancing element by element is the way.

Answer 9

OHH, so my answer is correct then? o:

Answer 10

yes

Answer 11

i mean you're answer lol

Answer 12

okay, ty!!! </333