00:02
Hello there for this question we see we have silver sulfide the tarnish on silver comes from the reaction of silver metal with hydrogen sulfide and oxygen gas so the first thing they want us to do is balance it so let's so to balance it we're going to count on each side each side to see if they are so we can determine whether if it's already balanced or not okay so let's let's do this so ag how many ag they are there is one while ag over here is two so we fix that then we see where h there is 2 h and we see the h here is also 2 so so this is good for our s on this side, there is one.
01:08
And our s on this side is also one.
01:13
So that's good.
01:14
So oxygen, we have two.
01:18
Let me fix it.
01:20
Two over here.
01:22
And how many oxygen we have over here? one.
01:26
So we see that our hydrogen, oxygen, i mean, our silver and our silver and our oxygen needs to be balanced.
01:41
So let's see we can fix this.
01:44
So we see that there is, so we see there's like two argon over here.
01:51
So we'll add two over here to balance it out.
02:00
And so for our hydrogen and our sulfide, they are good, but the oxygen, it needs to be two.
02:09
So to fix that we might have to add two here, but that's bad now because our s went from, i mean, our hydrogen went from being 2 to 4 and you know we could say that the oxygen is now too but now our hydrogen is at 4 so to fix that we might have to add 2 here which is also good because now we're at 4 but bad because now sulfide our sulfur now is 2 so to fix this so now to fix this we might have that need to add two over here which again fixes this where now this is two oops but now this now becomes four so how we're going to fix this we just go going to erase where which we originally had over here and just make it four and we have four here and looking at it all and all it's all balanced so we are good with that so now for the next one they want to know how many grams of sulfur sulfide can be formed from 496 grams of silver 80 grams of hydrogen sulfide and 40 grams of oxygen so how we're going to calculate this alright, so i wrote down the mass for each of them.
04:09
Oh, i forgot to write one for a silver.
04:12
Okay, now we got this silver.
04:15
So how we're going to go about calculating this? well, let's start with the first question where we have 496 silver, 96 grams.
04:35
And we're going to define this by the molar mass of the m -07 87, right ag.
04:50
So we know what we're crossing out.
04:56
And then let's go up to how many moles of silver we got.
05:01
So we see we have four.
05:02
So four moles of silver.
05:08
And this is how we're going to get to our ag.
05:11
Um a g um are silver sulfide which is um two okay come down come down okay two moles of a g of silver sulfide and then we're going to convert the moles back to grams because we're solving for grams so it's like one mole of a g to f f f f f f f is 247 .8 grams.
05:58
So look at all this and calculating all this, what should you get out of that setup? so the total you should get is 569 .7 grams of a sulfur sulfide.
06:29
So now since we saw for this one, can you solve for like the other two? i'll pause the video and we'll come back to see we both end up with the same answer.
06:43
Okay, so for the rest of them, so for the rest of them, like for the second part, if you hit your setup like this, then you did a good job that you put down the molar mass of our, our hydrogen sulfide and you put down the moles and you look up here how we balance them so that's why it's very important to balance them because they want to know basically how many grams of your byproduct that you got out from your product that you got from a certain amount let's say like 80 grams of hydrogen sulfide okay put down the mold there and we wrote down our molar mass from our product and that's how you should have 581 .3 grams of sulfur sulfide and then for the last one for oxygen you will have something set up like this and have this as your answer so then the next one they want to know which of the three reagents is the limiting reagents...