Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfuric acid. The unbalanced equation is
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2.49 g of copper(II) oxide is treated with 5.05 g of pure sulfuric acid, which reactant would limit the quantity of copper(II) sulfate that could be produced?
Interpretation:
The reactant that limits the quantity of copper (II) sulphate produced should be determined.
Concept Introduction:
Limiting reactant is the reactant that limits the amount of product formed in the chemical reaction. The mass of product formed from limiting reactant is theoretical yield which is less than the mass of product formed from the reactant in excess.
The balanced chemical reaction is as follows:
The mass of copper (II) oxide is 2.49 g and that of mass of pure sulphuric acid is 5.05 g. To determine the limiting reactant, first calculate the number of moles of copper (II) oxide and sulphuric acid as follows:
Molar mass of copper (II) oxide is 79.545 g/mol thus, number of moles will be:
Putting the values,
From the balanced chemical reaction, 1 mol of CuO gives 1 mol of
Since, molar mass of
Putting the values,
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