how many moles of iron oxide is required to produce 10 moles of carbon dioxide in the reaction 2Fe2 + c= Fe + 3CO2

Question

how many moles of iron oxide is required to produce 10 moles of carbon dioxide in the reaction 2Fe2O3 + c= Fe + 3CO2

Answer 1

the balanced equation for this reaction is

2Fe2​O3​ + 3C → 4Fe + 3CO2​

meaning that the mole ratio between iron oxide and carbon dioxide is 2:3

then you can use that value to scale it over

10 mol CO2 x 2 mol Fe2O3 / 3 mol CO2 = 6.67 mol Fe2O3

meaning that 6.67 moles of iron oxide are required to produce 10 moles of carbon dioxide

Answer 2

Let's just take this step by step.

Step 1: Understand the vocabulary. Mol is 6.022 x 10²³ pieces of a substance or molecule. It is similar in concept to a dozen.

Step 2: Look at the equation and mark what you need. Remember Iron Oxide is Fe2O₃ and Carbon Dioxide is CO₂.

2Fe2O3 + C= Fe + 3CO2 This is what the reaction is giving you but you need 10 mols (60.22 x 10²³)

So: if 2 Iron Oxides = 3 Carbon dioxides, then 2 mols of iron oxide = 3 mols of carbon dioxide.

Step 3: Set up an equivalency and solve.

2 Fe2O_{3 =. x.}

3 CO₂ 10 CO₂

So, 2 x 10 = 20/3 = 6 and 2/3 mols.