p.10-11Limiting and Excess Reactants/Reagents
Reaction between 2.50 g of aluminum and 375 mL of
0.10 M copper (II) sulphate pentahydrate solution
1.a) Write a balanced equation of this reaction
2Al(s) +3CuSO4•5H2O(aq) Al2(SO4)3(s) +3Cu(s)+15H2O(l)+ energy
b) Write the stoichiometric ratio
2 mol
3 mol
1 mol
3 mol
15 mol
c) n(Al) = 2.50 g X mol = 0.0926 mol Al
27.0 g
n(CuSO4•5H2O) = 0.1000 mol X 375 mL X 1 L
= 0.0375 mol
L
1000 mL
d) Predict the limiting and excess reactants:
limiting: reactant is completely used up at the end of the rxn
excess(xs): reactant is left over reactant at the end of the rxn
limiting: CuSO4•5H2O
used up
excess:
Al
left over
e) Write 3 chemical changes
colour change: turquoise to greyish colour
red solid is formed (Cu)
temperature is increased (exothermic)
2. How can we find the limiting reactant?
In order to find the limiting reactant, we do the following:
Road Map:
n(each reactant) n(one product)  mass(one product)
The winner (limiting reactant) is:
the reactant producing the least amount of product
3. Road map: p.11
mole
Have
bridge
X MM Want
n(reactants) ----- n(Cu) ----- xg(Cu) (product)
What is the limiting reactant?
(i) mass of copper produced from aluminum:
xg(Cu) = 0.0926 mol Al X 3 mol Cu X 63.5 g = 8.82 g Cu
reactant
2 mol Al mol Cu
(most)
(ii) mass of copper produced from copper(II)sulphate pentahydrate
xg(Cu) =
0.0375 mol CuSO4•5H2O X 3 mol Cu
X 63.5 g = 2.38 g Cu
reactant
3 mol CuSO4•5H2O mol Cu (least)
Winner, that is the limiting reactant, is: CuSO4•5H2O
4. What reactant is in excess? Al
5. How many moles of reactant are in excess?
n(Al)reacted:
limiting reactant
X reactants’ mole ratio= n (excess reactant)
0.0375molCuSO4•5H2OX 2 mol Al
= 0.0250mol Al reacted
3mol CuSO4•5H2O
n(Al)excess:
0.0926 mol (started)-0.0250 mol(reacted) =0.0676 mol in excess
4 dp
4 dp
4 dp and 3sf
6. Calculate the mass of reactant in excess?
n(xs)= 0.0676 mol
X 27.0 g = 1.83 g Al that didn’t react
mol
7. Find the mass of aluminum sulphate.
Road Map: n(limiting reactant)  n(product)  xg (product)
xg(Al2(SO4)3) =
0.0375 mol CuSO4•5H2O X 2 moles Al2(SO4)3 X 342.3 g = 8.56 g
3 moles CuSO4•5H2O mole Al2(SO4)3
8. Find the mass of copper produced.
xg(Cu) =
0.0375 mol CuSO4•5H2O X 3 moles Cu
X 63.5 g = 2.38 g
limiting reactant 3 moles CuSO4•5H2O mol Cu