00:01
Hello, so let's first look at the reaction.
00:04
So we got ion -3 nitrate plus 3 -k -o -h, that equals to 3k -0 -3 plus fe 0 -h.
00:37
So if you look at the more ratios here, you see that 1 mole of ion -3 nitrates is a reacting with 3 moles, right, of potassium hydroxide.
00:48
Produce 3 moles of k 103 so let's keep the more ratios in mind we're going to use that shortly before that let's look at the number of moles of f e and 03 which is the mass but the molar mass mass is 20 mona mass of ion of nitrate that's a constant that's 241 .599 the number of most of that is 0 .0 827.
01:39
Now look at the number of moles of potassium on the same formula mass is 17.
01:48
Malamass 86 .154.
01:57
Then 0 .30 .30 0 .30 most right now if you want to consume 17 grams of potassium address that the number of moles of ion nitrate required because you can see the more ratio is 1 is the 3 right so you need to really define the number of more of you know both right so let's see so zero let's look at this so 0 .0827 mo of f .e.
02:59
N .o .3.
03:03
That's going to be times 3 moles.
03:17
Potassium and peroxide, right? that's going to be divided by.
03:27
More of f .e.
03:32
N0 3.
03:35
That.
03:38
Okay.
03:42
So what is it going to be? so now the most of course this and this is going to cancel up.
03:50
So now the actual modes of this is going to react.
03:57
So most of koh reacted is going to be 0 .481.
04:20
So let's go back to the reaction.
04:22
See, look at this.
04:24
You realize that the number of moles of koh is more than that of ion nitrate.
04:32
So we need to recap, put it, to see the actual number of moles that reacted, i mean, the number of moles of potassium and droside, but that is more.
04:44
So we just found that...