Stiochemistry practice problems help

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To determine the moles of aluminum needed to form 3.4 moles of aluminum oxide, the balanced equation 4Al + 3O2 → 2Al2O3 indicates that 4 moles of aluminum produce 2 moles of aluminum oxide. This establishes a ratio of 4 moles of Al to 2 moles of Al2O3, simplifying to 2 moles of Al for every mole of Al2O3. To find the required moles of aluminum (x) for 3.4 moles of aluminum oxide, the equation can be set up as x/3.4 = 2/1. Understanding this ratio is crucial for solving the problem effectively. Mastery of balanced reaction equations is essential for tackling similar stoichiometry problems.
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Homework Statement



Aluminum oxide is formed from the reaction of metallic aluminum with oxygen gas. How many moles of Aluminum are needed to form 3.4 moles of Aluminum oxide?

Homework Equations



first equation:Al + O2 --> Al2O3 i balanced it at 4Al + 3O2 --> 2Al2O3

The Attempt at a Solution



okay I just really need help understanding this because I have no clue what I am doing and don't understand how to work the problem! please help:confused:
 
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Ok, so you've balanced your equation correctly. From this you know that 4 moles of aluminium produce 2 moles of aluminium oxide, and want to calculate the number of moles of Al required to produce 3.4 moles of aluminium oxide (x, say).

1. What is the ratio of Al to Al2O3?
2. Can you set up a ratio equation for x?
 
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