A student mixes an aqueous solution of \(\text{AgNO}_3\) with an aqueous solution of \(\text{MgCl}_2\), forming insoluble \(\text{AgCl(s)}\) according to the following balanced equation:

\[2\,\text{AgNO}_3\text{(aq)} + \text{MgCl}_2\text{(aq)} \rightarrow 2\,\text{AgCl(s)} + \text{Mg(NO}_3)_2\text{(aq)}\]

The particulate diagram represents the contents of the beaker after the reaction has gone to completion (solvent water molecules are omitted for clarity).

Based on the representation, what was the ratio of the initial number of moles of \(\text{AgNO}_3\) to the initial number of moles of \(\text{MgCl}_2\) present in the mixture before the reaction occurred?