Aluminum reacts with bromine to produce aluminum bromide according to the following equation: """2 al (s) + 3 br2 (l) => 2 albr3 (s)
in the lab you perform this reaction using an excess of aluminum and 55.7 grams of bromine. you end up
collecting 60.0 grams of product aluminum bromide. what is your percent yield?

iron reacts with oxygen to give iron(iii) oxide according to the following balanced equation: """4 fe (s) + 3 o2 (g) => 2 fe2o3 (s)"""
identify the limiting reactant in each of the following reactant mixtures:
a. 0.288 moles fe and 0.240 moles o2
b. 10.0 grams fe and 10.0 grams o2
c. 1.45 x 1024 atoms of fe and 7.21 x 1023 molecules of o2

sucrose (c12h22o11) reacts with potassium chlorate according to the following balanced equation: """c12h22o11 (s) + 8 kclo3 (s) => 12 co2 (g) + 11 h2o (g) + 8 kcl (s)"""
suppose 3.5 moles of c12h22o11 are mixed with 21.0 moles of kclo3. identify the limiting reactant, then
calculate how many moles of each product (co2, h2o and kcl) will be formed in this reaction.

boron trifluoride reacts with hydrogen according to the following balanced equation: """2 bf3 (g) + 3 h2 (g) => 2 b (s) + 6 hf (g)"""
suppose 40.00 grams of bf3 are mixed with 5.00 grams of h2.
a. identify the limiting reactant.
b. calculate the mass of hf generated.
c. calculate the mass of excess reactant that remains when the reaction is complete.
d. when this reaction is performed in the laboratory, the percent yield of hf is 72.6%. what was the
experimental yield of hf?

10. pure carbon reacts with sulfur dioxide gas producing liquid carbon disulfide and carbon monoxide gas.
a. write the balanced equation for this reaction.
b. what mass of carbon monoxide will be produced if 40.0 grams of carbon are allowed to react with 95.0 grams
of sulfur dioxide? what mass of excess reactant is left over?