00:02
Okay, let's go through this reaction first.
00:06
So it says for the sodium boronhydrate, you can use the reaction to produce that, which is you have the sodium hydride react with bromon hydride, right? and it will produce sodium boron hydride.
00:31
So you can actually balance it two and two.
00:36
And balanced.
00:38
So it says how many grams of the sodium bromohydride can be prepared by reaction between, let's see what it says by reaction between 8 .75 grams of the sodium hydride and 6 .9 grams of the bromohydride, and which one is a limiting agent? so first, let's see.
01:17
You can see that for the reaction you'll find every time you have two mores of the sodium hydride be consumed.
01:26
One more is a bromon hydride will also be consumed.
01:30
So the first thing we can calculate the mores of the sodium hydroxide and the mores of the sodium hydride and the mores of the boron hydrate.
01:42
So the more of the sodium hydride would be equal to the mass of the sodium hydroxide over the more mass here.
02:08
So the mass is 8 .75 and the more mass is actually around 24, right? so 8 .75 over 24 is equal to about 0 .3646 grams more.
02:31
And same, we can calculate the mores of the sodium, mores of the boron hydride, or boron hydrogen, would be equal to the mass 6 .9 over the more mass.
02:47
The more mass of the boron hydride would be equal to about 27 .622.
03:04
So the mores of the boron hydride would be equal to about, 0 .249a more.
03:30
As i mentioned, right, for a complete stymetric reaction, the more ratio of the sodium hydroxide, sodium hydride and the boron hydride is 2 to 1.
03:42
And if you look at that, you'll find that the ratio of sodium hydride is compared with the boron hydride is less than 2, which means the sodium hydride should be the limiting agent...