A student prepares a sample of magnesium sulfate crystals using this reaction:
MgO(s)+H2SO4(aq)→MgSO4(aq)+H2O(l) \text{MgO(s)} + \text{H}_2\text{SO}_4\text{(aq)} \rightarrow \text{MgSO}_4\text{(aq)} + \text{H}_2\text{O(l)} MgO(s)+H2SO4(aq)→MgSO4(aq)+H2O(l)She obtains the crystals from the solution formed.
She records this information about the reactants she uses:
(Relative atomic masses: Mg=24\text{Mg} = 24Mg=24, O=16\text{O} = 16O=16)
Calculate the amount, in moles, of magnesium oxide used.
Calculate the amount, in moles, of sulfuric acid used.
Why is it important for the amount of magnesium oxide to be greater than the amount of sulfuric acid?
State the name of the separation technique used to remove the excess magnesium oxide, and list two essential pieces of apparatus required.
In a similar preparation, the student uses 0.085 mol of magnesium oxide to obtain crystals of hydrated magnesium sulfate, MgSO4⋅7H2O\text{MgSO}_4 \cdot 7\text{H}_2\text{O}MgSO4⋅7H2O.
Calculate the maximum mass of MgSO4⋅7H2O\text{MgSO}_4 \cdot 7\text{H}_2\text{O}MgSO4⋅7H2O that she could obtain using this preparation.
(Relative atomic masses: H=1\text{H} = 1H=1, O=16\text{O} = 16O=16, Mg=24\text{Mg} = 24Mg=24, S=32\text{S} = 32S=32)
