Recap - Aluminum Plant

Part of the Stoichiometry section of Coddy's Chemistry journey. Lesson 28 of 41.

Challenge

An aluminum plant splits aluminum oxide with carbon blocks that burn away as it works: 2Al₂O₃ + 3C → 4Al + 3CO₂. In one day it is fed $20.4\ \mathrm{tons}$ of Al₂O₃ and $3.0\ \mathrm{tons}$ of carbon. What mass of aluminum can it make, in grams?

Try it yourself

Solve for $m_{Al}$

All lessons in Stoichiometry

1The Mole

Counting Particles: the Mole Avogadro's Number Molar Mass Mass, Moles and Particles Moles in a Formula Recap - Mole Bridge

4Equations and Mole Ratios

Balancing Equations Reading an Equation in Moles Mass to Mass Gas Volumes in Reactions Reactions in Solution Precipitation Recap - Rocket Fuel

2Gases

Molar Volume of a Gas Avogadro's Law Pressure, Volume, Temperature The Ideal Gas Law Recap - Weather Balloon

5Limiting Reactant

The Limiting Reactant What Is Left Over Industrial ScaleRecap - Aluminum Plant

3Solutions

Molar Concentration Preparing a Solution Ions in Solution Ion Concentrations Dilution Recap - Lab Prep

6Practice Problems

Recap - Fertilizer Plant Recap - Acid for the Plant Recap - Gases for Ammonia Recap - Ions in the Sample Recap - The Full Plant Recap - Bromide in Brine Recap - Chlorine for Bromine Recap - Magnesium Bromide Recap - Silver Bromide Test Recap - Balloon at Launch Recap - Balloon High Up Recap - Before It Bursts Recap - Hydrogen from Water