reactants that are not completely used up in a reaction are excess reagents
'' '' are completley used up '' '' limiting
Example
Finding Excess/Limiting Reagents
Find the limiting reagent and the reactant in excess when 0.5 moles of Zn react completely with 0.4 moles of HCl
Zn + 2HCl -----> ZnCl2 + H2
Compare the available moles of each reactant to the moles required for complete reaction using the mole ratio
Zn->HCl 0.5 x 2= 1.0 mole HCl
There are only 0.4 moles of HCl available which is less than the required 1.0 moles.
HCl->Zn 0.4 x 1 = 0.2 mols Zn
2
There are 0.5 moles of Zn available which is more than the required 0.2 moles.
The limiting reagent is HCl, Excess reagent= Zn
all of the 0.4 moles of HCl will be used up
when the reaction has gone to completion there will be
0.5 - 0.2 = 0.3 moles of Zn left over.
Example 2
Find the amount of H20 produced when 1.5g of CaCO3 react completely with 0.73g of HCl.
CaCO3 + 2HCl -----> CaCl2 + CO2 + H2O
1.5g CaCO3 x 1 x 18gH20 = 0.27g H20
100g
0.73gHCl x 1 x 1molH20 x 18gH20 = 0.18gH20
36.5g 2molHCl
Since HCl is the limiting reactant, you can only produce 0.18g of H20.