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

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :