00:01
Okay, so this problem, we're provided this reaction.
00:05
We're told that copper is reacting with silver nitrate.
00:08
We're told, oh, no, we're not told.
00:10
Since copper and silver are both cations, those cations are going to switch spots.
00:15
Therefore, we're going to produce silver and copper nitrate.
00:21
To balance this chemical reaction, we have to keep in mind that nitrate is minus one.
00:25
Copper is going to end up being plus two.
00:27
So when we do this, we need two agn -o -3, which means we need to.
00:31
To silver.
00:33
The question then asks us to determine the limiting reactant, which means we have to convert both of our reactants to the same unit.
00:43
Since this is asking us to determine the theoretical yield of silver, i'm going to convert both of them to silver, so i don't have to do more work.
00:52
Okay, so this is the reaction, so this is letter a.
00:58
So then letter b is determine the limiting reactant.
01:01
So we're going to convert both of these to grams of ag.
01:05
So we're going to start with our 7 .33 grams of copper.
01:09
If we start with grams of copper, grams of copper must go on the bottom.
01:15
And one mole of copper is going to go up top.
01:18
Also, i apologize, and i use are a little sloppy.
01:20
The molar mass of copper is 63 .55.
01:25
Then we're going to go mold a mole.
01:27
So we know that the moles of copper equals the moles of silver.
01:35
So when we have mole on top of mole, we need to look at the coefficients.
01:38
The coefficient of silver is two, while the coefficient of copper is one.
01:43
Last but not least, we need to multiply by mass.
01:46
So we know that one mole of silver has a molar mass displayed on the periodic table, which is 107 .87.
01:59
So when we do this, we're going to go 7 .33...