You would see
So, you're basically dealing with a double replacement reaction which leads to the formation of a white precipitate, silver chloride. The balanced chemical equation for this reaction looks like this
In an ideal scenario, you'll have enough moles of both reactants so that neither of them can act as a limiting reagent. You can determine if this is the case by calculating how many moles of each reactant you get - use their molar masses
This shows that you have insufficient moles of silver nitrate to allow for all the moles of sodium chloride to react
Since only 0.0883 moles of each reactant will actually react, the number of moles of silver chloride and sodium nitrate produced will be equal to 0.0883.
The masses produced will be
The total mass produced will be
This is equal to the total mass that reacted, which is
Keep in mind that this is your theoretical yield - the amount produced when the reaction has a 100% yield.