This question is about magnesium and compounds of magnesium.
A student produces pure crystals of magnesium sulfate by reacting magnesium oxide with sulfuric acid.
The equation for the reaction is: 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)
The student adds magnesium oxide to sulfuric acid until the magnesium oxide is in excess. Give one observation that the student could make to show that the magnesium oxide is in excess.
Why is excess magnesium oxide used rather than excess sulfuric acid?
Name one other magnesium compound that the student could add to sulfuric acid to produce magnesium sulfate.
Describe how the student should obtain crystals of magnesium sulfate from a solution of magnesium sulfate.
Magnesium sulfate is also produced in a displacement reaction between magnesium and copper sulfate solution.
The equation for the reaction is: Mg+CuSO4→MgSO4+Cu\text{Mg} + \text{CuSO}_4 \rightarrow \text{MgSO}_4 + \text{Cu}Mg+CuSO4→MgSO4+Cu
Complete the ionic equation for this displacement reaction: Mg+‾→Mg2++‾\text{Mg} + \underline{\qquad\qquad} \rightarrow \text{Mg}^{2+} + \underline{\qquad\qquad}Mg+→Mg2++
Why is magnesium described as being oxidised in this reaction?