How Many Moles Of Aluminum Are Needed To React Completely With 2.1 Moles Of FeO? 2Al(s) + 3FeO(s) → 3Fe(s)
Understanding chemical reactions and stoichiometry is fundamental in chemistry, especially when determining how much of a reactant is needed to fully convert another reactant into a desired product. In this case, we are asked to find out how many moles of aluminum (Al) are required to completely react with 2.1 moles of iron(II) oxide (FeO) based on the balanced chemical equation:
\[ 2 \text{Al} (s) + 3 \text{FeO} (s) \rightarrow 3 \text{Fe} (s) \]
This question involves applying the principles of molar ratios and stoichiometry, which are essential tools in quantitative chemistry. To answer this, we will explore the reaction in detail, understand the molar relationships, and perform the necessary calculations to determine the exact amount of aluminum required.
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Understanding the Balanced Chemical Equation
Reaction Components
The reaction involves three substances:
- Aluminum (Al): a metal that acts as a reducing agent.
- Iron(II) oxide (FeO): an oxide of iron, serving as the oxidizing agent.
- Iron (Fe): the product of the reduction of FeO.
The balanced equation:
\[ 2 \text{Al} (s) + 3 \text{FeO} (s) \rightarrow 3 \text{Fe} (s) \]
This indicates that:
- 2 moles of aluminum react with 3 moles of FeO.
- The reaction produces 3 moles of iron.
From the coefficients, the molar ratio of Al to FeO is 2:3.
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Determining the Molar Ratio
Significance of the Coefficients
Coefficients in a balanced chemical equation provide the molar ratios of reactants and products involved in the reaction. For our reaction:
- For every 2 moles of Al, 3 moles of FeO are consumed.
- This ratio can be written as:
\[ \frac{\text{Moles of Al}}{\text{Moles of FeO}} = \frac{2}{3} \]
or equivalently:
\[ \text{Moles of Al} = \frac{2}{3} \times \text{Moles of FeO} \]
This relationship allows us to convert between quantities of different reactants.
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Calculating the Moles of Aluminum Needed
Given Data
- Moles of FeO = 2.1 mol
Calculation Steps
- Set up the molar ratio relation:
- Plug in the given value:
- Perform the multiplication:
- Simplify:
Result: To react completely with 2.1 moles of FeO, 1.4 moles of aluminum are required.
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Additional Considerations in Stoichiometry
Reaction Conditions
While calculations provide the theoretical amount of reactants needed, real-world reactions may be influenced by:
- Reaction completeness: Is the reaction going to go to completion under the given conditions?
- Purity of reactants: Impurities may affect the amount of reactant needed.
- Reaction environment: Temperature, pressure, and catalysts can influence reaction efficiency.
Limiting Reactant Concept
In practical scenarios, identifying the limiting reactant is crucial. Since the problem specifies the amount of FeO and asks for the required aluminum, it assumes aluminum is in excess or that FeO is the limiting reactant.
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Understanding Stoichiometry in Depth
Stoichiometry as a Tool
Stoichiometry allows chemists to:
- Calculate the exact quantities of reactants needed for a desired reaction.
- Predict the amount of products formed.
- Determine the efficiency of reactions.
Practical Applications
This calculation is not just theoretical but has real-world applications such as:
- Manufacturing processes involving metals.
- Designing chemical reactors.
- Ensuring efficient use of raw materials in industrial production.
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Summary of Key Points
- The balanced chemical equation provides the molar ratio between aluminum and FeO as 2:3.
- To find the moles of aluminum needed for 2.1 mol of FeO, we use the ratio: \(\text{Al} = \frac{2}{3} \times \text{FeO}\).
- The calculation yields 1.4 moles of aluminum required.
- Understanding molar ratios is essential for accurate stoichiometric calculations.
- Real-world considerations may influence the actual quantity needed, but the theoretical calculation provides a baseline.
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Conclusion
In summary, based on the stoichiometry of the reaction between aluminum and iron(II) oxide, 1.4 moles of aluminum are required to completely react with 2.1 moles of FeO. This calculation underscores the importance of balanced chemical equations and molar ratios in quantitative chemistry. By mastering these principles, chemists can precisely compute reactant requirements, optimize chemical processes, and ensure efficient resource utilization in various industrial and laboratory settings.
