We appreciate your visit to How many grams of Al are needed to completely react with 135 g of tex text Fe 2 text O 3 tex. This page offers clear insights and highlights the essential aspects of the topic. Our goal is to provide a helpful and engaging learning experience. Explore the content and find the answers you need!
Answer :
About 45.6 gAL are need to completely react with 135g FE2O3
Thanks for taking the time to read How many grams of Al are needed to completely react with 135 g of tex text Fe 2 text O 3 tex. We hope the insights shared have been valuable and enhanced your understanding of the topic. Don�t hesitate to browse our website for more informative and engaging content!
- Why do Businesses Exist Why does Starbucks Exist What Service does Starbucks Provide Really what is their product.
- The pattern of numbers below is an arithmetic sequence tex 14 24 34 44 54 ldots tex Which statement describes the recursive function used to..
- Morgan felt the need to streamline Edison Electric What changes did Morgan make.
Rewritten by : Barada
To determine the mass of Al needed to react with 135 grams of Fe₂O₃, convert the mass of Fe₂O₃ to moles, use the stoichiometric ratio to find moles of Al needed, and then convert those moles to grams of Al to three significant figures.
The question is asking how many grams of aluminum (Al) are needed to completely react with 135 grams of iron(III) oxide (Fe2O3). This is a stoichiometry problem that requires using the balanced chemical equation:
Fe₂O₃(s) + 2Al(s) →2Fe(s) + Al₂O₃(s)
We start by converting the mass of Fe₂O₃ to moles using its molar mass:
1.0g Fe₂O₃ / 159.7 g/mol = moles of Fe₂O₃
Then we use the mole ratio from the balanced equation to convert from moles of Fe₂O₃ to moles of Al. The molar mass of Al is 27.0 g/mol. Finally, we convert moles of Al to grams using its molar mass to find the mass of Al needed for the reaction.
With the provided mass of 135g of Fe₂O₃, and the reaction stoichiometry, we can determine the mass of Al required which will be expressed to three significant figures.
