Answer:
1.) 2 Fe (s) + 3 Cl₂ (g) ---> 2 FeCl₃ (aq)
2.) 2.0 moles FeCl₃
3.) 0.67 moles FeCl₃
4.) 1.5 g FeCl₃
Explanation:
1.)
The unbalanced reaction:
Fe (s) + Cl₂ (g) ---> FeCl₃ (aq)
<u>Reactants</u>: 1 iron, 2 chlorine
<u>Products</u>: 1 iron, 3 chlorine
The balanced reaction:
2 Fe (s) + 3 Cl₂ (g) ---> 2 FeCl₃ (aq)
<u>Reactants</u>: 2 iron, 6 chlorine
<u>Products</u>: 2 iron, 6 chlorine
2.)
To find moles FeCl₃, you need to multiply the given value by the mole-to-mole ratio of Fe to FeCl₃. This ratio is constructed via the coefficients from the balanced equation.
2.0 moles Fe 2 moles FeCl₃
--------------------- x ------------------------ = 2.0 moles FeCl₃
2 moles Fe
3.)
To determine how much FeCl₃ is produced, you need to identify the limiting reagent. To find it, you need to convert both reactants to the product then identify which reactant gives you the smallest amount of product. This reactant is the limiting reagent and will give you your actual answer.
1.0 mole Fe 2 moles FeCl₃
------------------- x ----------------------- = 1.0 moles FeCl₃
2 moles Fe
1.0 mole Cl₂ 2 moles FeCl₃
------------------- x ------------------------ = <u>0.67 moles FeC</u>l₃
3 moles Cl₂
4.)
Because Cl₂ is the limiting reagent, we need to convert grams Cl₂ to grams FeCl₃. This can be done using the molar masses of both compounds and the mole-to-mole ratio.
Molar Mass (Cl₂): 2(35.453 g/mol)
Molar Mass (Cl₂): 70.906 g/mol
Molar Mass (FeCl₃): 55.845 g/mol + 3(35.453 g/mol)
Molar Mass (FeCl₃): 162.204 g/mol
1.0 g Cl₂ 1 mole 2 moles FeCl₃ 162.204 g
------------- x ----------------- x ----------------------- x ------------------ = 1.5 g FeCl₃
70.906 g 3 moles Cl₂ 1 mole
