AQA GCSE Chemistry

Revision Notes

3.3.2 Theoretical Masses of Products

Higher Tier Only

Obtaining Calculated Masses

  • We can obtain theoretical masses of products using a balanced equation and a given mass of reactant
  • The process is as follows:
    1. Write out the balanced equation for the reaction(if not already given in the question)
    2. Convert the given mass of reactant(s) into moles, by dividing the masses by the molar masses
    3. Use the coefficients(multipliers) in the equation to deduce the number of moles of the product(s)
    4. Convert the moles of product into mass by multiplying by the molar mass
  • The following example illustrates the process:

Worked Example

In an experiment to displace copper from copper(II)sulfate, 6.5g of zinc was added to a solution of copper(II)sulfate. The copper was filtered off, washed, dried and weighed. the final mass of copper obtained was 4.8 g. Calculate the percentage yield of copper.

The balanced equation for the reaction is

Zn (s) + CuSO4 (aq)  ⟶ Cu (s) + ZnSO4 (aq)

Answer

Percentage Yield WE Answer, downloadable IGCSE & GCSE Chemistry revision notes

Exam Tip

The key to success in all calculations is to have a methodical step-by-step approach and show all your workings. Be careful when working out the molar masses not to include coeffiecients. It is very easy to make the mistake of calculating the molar mass of magnesium oxide as 80 g instead of 40 g, when working from an equation:

2Mg (s) + O(g) → 2MgO (s)

(Mg = 24 g mol−1; O = 16 g mol−1 )

Remember that molar masses are calculated from chemical formulae, not from equations

Author: Francesca

Fran has taught A level Chemistry in the UK for over 10 years. As head of science, she used her passion for education to drive improvement for staff and students, supporting them to achieve their full potential. Fran has also co-written science textbooks and worked as an examiner for UK exam boards.
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