We can represent the oxidation so..........
$Mg(s) +1/2O_2(g) stackrel(Delta)rarrMgO(s)$
And thus combustion of one equiv magnesium metal, $24.3*g$, should lead to formation of approx. $40*g$ magnesium oxide. And thus the mass contained by the crucible should almost double.
Often when you do the experiment, you lose some of mass, i.e. the $MgO$ ash is lost from the crucible. Be careful and don't burn yourself on the crucible.