Question #289b9
1 Answer
Here's what I got.
Explanation:
Let's take a look at the first half-reaction
#"H"_ (2(g)) -> 2"H"_ ((aq))^(+) + 2"e"^(-)#
Notice that hydrogen gas,
In other words, you can say that the above half-reaction describes the oxidation of molecular hydrogen to hydrogen ions.
Move on to the second half-reaction.
#1/2"O"_ (2(g)) + 2"H"_ ((aq))^(+) + 2"e"^(-) -> "H"_ 2"O"_ ((l))#
This time, you have electrons added to the products' side, so right from the start, you can say that this represents a reduction half-reaction.
Since you're dealing with a half-reaction, only one element will change its oxidation state. In this case, hydrogen is present as ions on the products' side, which implies an oxidation state of
On the products' side, hydrogen is once again in a
You can thus say that this half-reaction describes the reduction of molecular oxygen to water; as a result, oxygen's oxidation state decreases from
#1/2 stackrel(color(blue)(0))("O") _ (2(g)) + 2"H"_ ((aq))^(+) + 2"e"^(-) -> "H"_ 2 stackrel(color(blue)(-2))("O") _ ((l))#
Finally, look at the third half-reaction.
#"Cd"_ ((s)) + 2"OH"_ ((aq))^(-) -> "Cd"("OH") _(2(s)) + 2"e"^(-)#
Once again, the electrons are added to the products' side, so you know that an element is losing electrons
More specifically, cadmium,