A technician adds excess iron powder to a used copper sulfate solution so that copper can be recovered.
Fe(s)+CuSO4(aq)→FeSO4(aq)+Cu(s)\mathrm{Fe(s) + CuSO_4(aq) \rightarrow FeSO_4(aq) + Cu(s)}Fe(s)+CuSO4(aq)→FeSO4(aq)+Cu(s)
Relative formula mass: CuSO4=160\mathrm{CuSO_4} = 160CuSO4=160
Relative atomic mass: Cu=64\mathrm{Cu} = 64Cu=64
The solution contains 8.00 g of copper sulfate in 250 cm3 of solution. The iron is in excess, so all the copper sulfate reacts.
Calculate the volume of the copper sulfate solution in dm3\mathrm{dm^3}dm3.
Use your answer to (a) to calculate the concentration of copper sulfate in the solution. Give your answer in g dm−3\mathrm{g\,dm^{-3}}gdm−3.
Calculate the mass of copper produced when all the copper sulfate reacts.
The solids are filtered off. The filtrate contains 7.60 g of iron sulfate.
Water is added to the filtrate until the concentration of iron sulfate is 15.2 g dm−315.2\ \mathrm{g\,dm^{-3}}15.2 gdm−3.
Calculate the total volume of the solution after the water is added.
142 exam-style questions on Edexcel GCSE Chemistry 2.6 Calculations involving masses, covering 2.6.1 Relative formula mass and percentage composition, 2.6.2 Empirical and molecular formulae, 2.6.3 Conservation of mass, 2.6.4 Reacting masses and concentration in g dm⁻³, 2.6.5 The mole and the Avogadro constant, and 2.6.6 Limiting reactants and stoichiometry. Each one has a worked solution and a mark scheme showing where the marks go.