For the following reaction, 0.429 moles of iron(II) chloride are mixed with 0.190 moles of silver nitrate.?

Initial amount of FeCl₂ = 0.429 mol
Initial amount of AgNO₃ = 0.190 mol

The equation for the reaction :
FeCl₂(aq) + 2AgNO₃(aq) → Fe(NO₃)₂(aq) + 2AgCl(aq)
Mole ratio FeCl₂ : AgNO₃ = 1 : 2

If AgNO₃ complete reacts, amount of FeCl₂ needed = (0.190 mol) × (1/2) = 0.095 mol < 0.429 mol
Hence, FeCl₂ is in excess.
The formula for the limiting reagent : AgNO₃

Refer to the above equation, mole ratio AgNO₃ : Fe(NO₃)₂ = 2 : 1
Amount of AgNO₃ reacted = 0.190 mol
Maximum amount of Fe(NO₃)₂ produced = (0.190 mol) × (1/2) = 0.095 mol