We got to see what happens in a chemical reaction when the limiting reactant runs out (the reaction stops). We learned about percent yield and worked some practice problems,
Homework:
from page 6-10 work #9-10 (we updated the questions slightly); see the updated versions below:
9.Sulfuric acid reacts with aluminum hydroxide by double replacement.
3H2SO4 + 2Al(OH)3 ® Al2(SO4)3 + 6H2O
If 750.0 mL of 3.00 M sulfuric acid react with 900.0 mL of a 2.70 M of aluminum hydroxide:
a.)What is the limiting reactant?
b.)What is the theoretical yield of aluminum sulfate in grams?
c.)How much excess, in grams, remains?
d.)How many grams of aluminum sulfate would be made if the reaction only has a 65.4% yield?
10.The compound SF6 is made by burning sulfur in an atmosphere of fluorine. The balanced equation is:
S8(s) + 24 F2 (g) ® 8SF6(g)
In a reaction between 80.0 grams of octasulfur and 160.0 grams of fluorine:
a.)Which is the limiting reactant?
b.)How many liters of SF6 could be produced at STP, assuming 85% yield?
c.) How many grams of the excess reagent would be left over? (Ignore the % yield.)
Homework:
from page 6-10 work #9-10 (we updated the questions slightly); see the updated versions below:
9.Sulfuric acid reacts with aluminum hydroxide by double replacement.
3H2SO4 + 2Al(OH)3 ® Al2(SO4)3 + 6H2O
If 750.0 mL of 3.00 M sulfuric acid react with 900.0 mL of a 2.70 M of aluminum hydroxide:
a.)What is the limiting reactant?
b.)What is the theoretical yield of aluminum sulfate in grams?
c.)How much excess, in grams, remains?
d.)How many grams of aluminum sulfate would be made if the reaction only has a 65.4% yield?
10.The compound SF6 is made by burning sulfur in an atmosphere of fluorine. The balanced equation is:
S8(s) + 24 F2 (g) ® 8SF6(g)
In a reaction between 80.0 grams of octasulfur and 160.0 grams of fluorine:
a.)Which is the limiting reactant?
b.)How many liters of SF6 could be produced at STP, assuming 85% yield?
c.) How many grams of the excess reagent would be left over? (Ignore the % yield.)