Answer:
Iron is limiting reactant
Explanation:
Based on the reaction:
Fe + S → FeS
1 mole of iron reacts per mole of Sulfur
To solve this question we must convert the mass of each reactant to moles using molar masses of each reactant. As the reaction is 1:1, the reactant with the lower amount of moles is limiting reactant.
Moles Fe -Molar mass: 55.845g/mol-
4.68g * (1mol / 55.845g) = 0.0838 moles
Moles S -Molar mass: 32.065g/mol-
2.88g * (1mol / 32.065g) = 0.0898 moles
As the amount of moles of Fe < Moles S,
Iron is limiting reactant
When 4.68 g of iron reacts with 2.88 g of sulfur to produce FeS, iron is the limiting reagent.
If in a chemical reaction two reactants are present and one of them is present in less quantity as compared to other, is known as limiting reagent.
Given chemical reaction is:
Fe + S → FeS
From the stoichiometry of the reaction it is clear that equal moles of both reactant is required for the formation of product, so their mole ratio is 1:1.
Now we calculate the moles by using the formula:
n = W/M, where
W = given mass
M = molar mass
Moles of 4.68g of iron = 4.68g / 55.845g/mole = 0.0838 moles
Moles of 2.88 of sulfur = 2.88g / 32.065g/mole = 0.0898 moles
Moles of iron is less as compare to the sulfur, so it is the limiting reagent.
Hence, iron is the limiting reagent.
To know more about limiting reagent, visit the below link:
https://brainly.com/question/14222359
