Pure iron, Fe, can be produced from an ore called hematite, Fe, O,, by reaction with carbon at high temperatures. 2 Fe, O, +3C → 4 Fe + 3 CO, How many tons of hematite must react with carbon if an iron company needs to make 57 tons of iron? tons Fe,0,

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I very confused mid way in the equation when trying to do conversions.
**Topic: Production of Pure Iron from Hematite Ore**

In metallurgy, pure iron (Fe) can be extracted from an ore known as hematite, which is iron(III) oxide (Fe₂O₃). This extraction involves a chemical reaction with carbon (C) at high temperatures. The balanced chemical equation for this reaction is:

\[ 2 \text{Fe}_2\text{O}_3 + 3 \text{C} \rightarrow 4 \text{Fe} + 3 \text{CO}_2 \]

**Problem Statement:**

Determine how many tons of hematite (Fe₂O₃) are required to react with carbon if an iron company needs to produce 57 tons of pure iron (Fe).

**Answer Box:**

\[ \_\_\_ \text{ tons Fe}_2\text{O}_3 \]

This problem involves stoichiometry principles, requiring the use of molar ratios from the balanced equation to solve for the amount of hematite needed.
Transcribed Image Text:**Topic: Production of Pure Iron from Hematite Ore** In metallurgy, pure iron (Fe) can be extracted from an ore known as hematite, which is iron(III) oxide (Fe₂O₃). This extraction involves a chemical reaction with carbon (C) at high temperatures. The balanced chemical equation for this reaction is: \[ 2 \text{Fe}_2\text{O}_3 + 3 \text{C} \rightarrow 4 \text{Fe} + 3 \text{CO}_2 \] **Problem Statement:** Determine how many tons of hematite (Fe₂O₃) are required to react with carbon if an iron company needs to produce 57 tons of pure iron (Fe). **Answer Box:** \[ \_\_\_ \text{ tons Fe}_2\text{O}_3 \] This problem involves stoichiometry principles, requiring the use of molar ratios from the balanced equation to solve for the amount of hematite needed.
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