Stoichiometry \# 1 Directions: Be sure to show all work. Use units and sig figs on your final answer. Equation for questions 1-4: \[ 4 \mathrm{Al}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3} \] 1. How many grams of aluminum oxide would form if 12.5 moles of aluminum burned? 2. How many moles of oxygen are needed to react with 7.5 moles of aluminum? 3. How many moles of oxygen are needed to react with 100.0 grams of aluminum? 4. How many grams of aluminum burned if 200.0 grams of aluminum oxide formed?
Added by David M.
Close
Step 1
To find the grams of aluminum oxide formed, we need to use the molar mass of aluminum oxide (Al2O3). The molar mass of Al2O3 is 101.96 g/mol. First, we need to find the moles of aluminum (Al) in 12.5 moles of aluminum. Since the coefficient of Al in the balanced Show more…
Show all steps
Your feedback will help us improve your experience
Hitendra Singh and 57 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Aluminum metal reacts with oxygen to produce aluminum oxide: 4Al(s) + 3O2(g) → 2Al2O3(s). Calculate the mass of Al2O3 that will be produced if the reaction of 125 g of aluminum and sufficient oxygen has a 75.0% yield. Be sure to use full calculations and correct sig figs.
Hitendra S.
Aluminum reacts with oxygen to give aluminum oxide. $$ 4 \mathrm{Al}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(\mathrm{~s}) $$ If you have $6.0$ mol Al, how many moles and how many grams of $\mathrm{O}_{2}$ are needed for complete reaction? What mass of $\mathrm{Al}_{2} \mathrm{O}_{3}$, in grams, is produced?
Consider the balanced chemical equation $$4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{Al}_{2} \mathrm{O}_{3}(s)$$ What mole ratio would you use to calculate how many moles of oxygen gas would be needed to react completely with a given number of moles of aluminum metal? What mole ratio would you use to calculate the number of moles of product that would be expected if a given number of moles of aluminum metal reacts completely?
Chemical Quantities
The Concept of Limiting Reactants
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Watch the video solution with this free unlock.
EMAIL
PASSWORD