In reality, reactants don't have to react in perfect whole-numbers of moles. In a two-reactant synthesis reaction, usually one reactant gets entirely used up (and determines how much product is made), even if that means using fractions of a
mole of reactant. For instance, when solid, metallic aluminum Al and red, liquid bromine Bry are brought together, they
make a white solid according to the reaction 2. Al + 3 Br, → 2 AIBr, If 5.0 moles of aluminum Al was reacted with 10
moles bromine Bry, all five moles of aluminum would react, with only 7.5 moles bromine. (2:3 mole ratio) This would
produce only 5.0 moles of AIBr;, leaving 2.5 moles of excess Br, behind.
6. Now assume 3 moles Al and 4 moles Br2 react
a)Which chemical is the limiting reactant?
b)Which chemical must be the excess reactant?
b)
c)
c)How much (in moles) AIBr; gets produced?
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d)
d)If all the limiting reactant gets used up, how much of the excess reactant is left?
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7. What is the maximum amount (in moles) of NaCl that can be produced from 4.5 moles of Na and 3.5 moles of Cl2
according to the reaction Na +_ Cl, → _NaCl (left for you to balance).
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7).
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