A student prepares a sample of copper(II) sulfate crystals using this reaction:
CuO(s)+H2SO4(aq)→CuSO4(aq)+H2O(l) \text{CuO(s)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{CuSO}_4\text{(aq)} + \text{H}_2\text{O(l)} CuO(s)+H2SO4(aq)→CuSO4(aq)+H2O(l)She obtains the crystals from the solution formed.
She records this information about the reactants she uses:
(Relative atomic masses: Cu=64\text{Cu} = 64Cu=64, O=16\text{O} = 16O=16)
Calculate the amount, in moles, of copper(II) oxide used.
Calculate the amount, in moles, of sulfuric acid used.
Why is it important for the amount of copper(II) oxide to be greater than the amount of sulfuric acid?
State the name of the separation technique used to remove the excess copper(II) oxide, and list two essential pieces of apparatus required.
In a similar preparation, the student uses 0.056 mol0.056\text{ mol}0.056 mol of copper(II) oxide to obtain crystals of hydrated copper(II) sulfate, CuSO4⋅5H2O\text{CuSO}_4 \cdot 5\text{H}_2\text{O}CuSO4⋅5H2O.
Calculate the maximum mass of CuSO4⋅5H2O\text{CuSO}_4 \cdot 5\text{H}_2\text{O}CuSO4⋅5H2O that she could obtain using this preparation.
(Relative atomic masses: H=1\text{H} = 1H=1, O=16\text{O} = 16O=16, S=32\text{S} = 32S=32, Cu=64\text{Cu} = 64Cu=64)
