iron (iii) oxide reacts with solid carbon in the followed reaction: 2fe2o3(s) + 3c(s) → 4fe(s) + 3co2(g) what mass of fe2o3 is necessary to produce 100. l of co2 at 300. k and 2.10 atm? 823 g fe2o3 908 g fe2o3 1,110 g fe2o3 1,360 g fe2o3

908 g Fe₂O₃

General Formulas and Concepts:

Chemistry - Gas Laws

Combined Gas Law: PV = nRT

Chemistry - Stoichiometry

Explanation:

Step 1: Define

[RxN]   2Fe₂O₃ (s) + 3C (s) → 4Fe (s) + 3CO₂ (g)

[Given]   100 L CO₂ at 300 K and 2.10 atm

Step 2: Find Moles

Apply the Combined Gas Law and solve.

Step 3: Identify Conversions

[RxN]   3 mol CO₂ = 2 mol Fe₂O₃

Molar Mass of Fe - 55.85 g/mol

Molar Mass of O - 16.00 g/mol

Molar Mass of Fe₂O₃ - 2(55.85) + 3(16.00) = 159.7 g/mol

Step 4: Stoichiometry

= 907.755 g Fe₂O₃

Step 5: Check

We are given 3 sig figs. Follow sig fig rules and round.

907.755 g Fe₂O₃ ≈ 908 g Fe₂O₃