I can't figure this out and it's bothering me!
When 9.00g of Al reacts with an excess of H3PO4, 30.00g of AlPO4 is produced. What is the percent yield for this reaction?
When 9.00g of Al reacts with an excess of H3PO4, 30.00g of AlPO4 is produced. What is the percent yield for this reaction?
-
1 mole Al = 27g
X = 9g
X = 0.3333
I mole AlPO4 = 27 + 31 + 16 + 16 + 16 +16
1 mole = 122g
0.333 = 40.626g
So theoretical yield is 40.626g
We made 30g
Percentage yield = what we got/what we should have got
=30/40.626 x100%
= 73.8%
Hope that makes sense?
The limiting reagent (the one that's not in excess) determines the molarity of the product!
Good luck :)
X = 9g
X = 0.3333
I mole AlPO4 = 27 + 31 + 16 + 16 + 16 +16
1 mole = 122g
0.333 = 40.626g
So theoretical yield is 40.626g
We made 30g
Percentage yield = what we got/what we should have got
=30/40.626 x100%
= 73.8%
Hope that makes sense?
The limiting reagent (the one that's not in excess) determines the molarity of the product!
Good luck :)