00:01
For this question, we have a reaction between silver nitrate and sodium chloride to produce silver chloride and sodium nitrate.
00:07
And we want to know what is the theoretical yield of silver chloride? and then we want to know which reactant is limiting.
00:13
And then finally, we want to know if 1 .84 grams of silver chloride was actually produced in the lab.
00:19
What's the percent yield? so for this, we're going to have two different setups converting from each of our reactants to silver chloride.
00:25
And then we'll talk about how to determine the theoretical yield from there.
00:28
And then after that we will move on to percent yield.
00:31
So we're first going to start with our 3 .10 grams of silver nitrate that was given to us in the problem.
00:39
And we're going to convert to silver chloride.
00:41
So we first have to use silver nitrate's molar mass.
00:45
So we're going to have one mole of silver nitrate on top.
00:48
And then it's molar mass on the bottom, which is 169 .87 grams.
00:56
We're then going to use a mole ratio to get to silver chloride.
00:59
These numbers just come from your balanced chemical reaction.
01:01
So we've got one mole of silver chloride on top and one mole of silver nitrate on the bottom.
01:10
And then finally we're going to have silver chloride's molar mass.
01:12
So we can get to grams.
01:14
So we'll have 143 .32 grams of silver chloride on top over one mole of silver chloride.
01:24
So we multiply everything across the top and then divide by the things on the bottom.
01:28
And our first possible theoretical yield is 2 .62 grams of silver chloride.
01:36
So now we're going to do the same thing converting from sodium chloride to silver chloride...