How many molecules of carbon would I need to react completely with 2.34x10^{4} molecules of iron (III) oxide? Enter your answer as a whole number using the correct number of significant figures. Do NOT use scientific notation.

The reaction between carbon and iron(III) oxide (Fe₂O₃) typically proceeds as:

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

From this balanced equation, 1 molecule of Fe₂O₃ reacts with 3 molecules of carbon (C). 

Given:
- You have \(2.34 \times 10^4\) molecules of iron(III) oxide.
- The ratio of Fe₂O₃ to C is 1:3, meaning 1 molecule of Fe₂O₃ needs 3 molecules of carbon to react completely.

### Calculation:
To find how many molecules of carbon are needed:

\[
\text{Molecules of C} = 3 \times (2.34 \times 10^4)
\]
\[
\text{Molecules of C} = 7.02 \times 10^4 \text{ molecules of carbon}
\]

Thus, the total number of carbon molecules needed is **70,200 molecules**.

Would you like more details or have any further questions?

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Here are some related questions:
1. What is the role of carbon in this reaction?
2. How do you determine the limiting reagent in reactions like this?
3. What are the products formed in this reaction?
4. How can we convert molecules into moles in such reactions?
5. How do significant figures affect the accuracy of the result?

**Tip:** Always check the balanced chemical equation to understand the stoichiometric relationship between reactants.

This problem explores the stoichiometric relationship between carbon and iron(III) oxide (Fe₂O₃), using significant figures to determine how many molecules of carbon are required to react with 2.34x10^4 molecules of iron(III) oxide. The balanced chemical equation shows the 1:3 ratio between Fe₂O₃ and C, resulting in 70,200 molecules of carbon required for complete reaction.

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