Use the equation below to answer the following question: Fe+Cl2-->FeCl2 A student wants to prove the concept of limiting reactants to his labmates during class. If the student adds 56 g of Fe to 71 g of Cl2, what will the likely result of the reaction be in regards to limiting/excess reactants? Question 1 options: Although there is more Cl2, it takes two chlorine atoms to react with every one iron atom, so iron will be the excess reagent and chlorine will be the limiting reagent. There is an equal amount of iron and chloride; however, because of the 1:2 Fe:Cl nature of the reaction, iron will be in excess and chlorine will be the limiting reagent. Because there is more Cl2, chlorine will be the excess reagent and iron will be the limiting reagent. Based on the balanced equation, there is an equal amount of iron and chloride, so the reactants will be fully consumed with neither limiting nor in excess.