If you have 4.00 moles Al(aluminum), how many moles of O (oxygen)subscript 2 are needed for a complete reaction?
Write the balanced equation.
4Al + 3O2 ==> 2Al2O3
Therefore, the equation tells us that 4 moles Al will require 3 moles O2.
To determine the moles of O₂ needed for the complete reaction with 4.00 moles of Al (aluminum), we need to use the balanced chemical equation.
The balanced chemical equation for the reaction between aluminum and oxygen is:
4 Al + 3 O₂ → 2 Al₂O₃
From the equation, we can see that 4 moles of Al react with 3 moles of O₂ to produce 2 moles of Al₂O₃.
Therefore, if we have 4.00 moles of Al, we can use a mole ratio to find the moles of O₂ needed:
(4 moles Al) / (4 moles Al₂O₃) × (3 moles O₂) = 3.00 moles O₂
So, 3.00 moles of O₂ are needed for a complete reaction with 4.00 moles of Al.
To determine the number of moles of O2 needed for a complete reaction with 4.00 moles of Al, we need to consider the balanced chemical equation for the reaction.
The balanced equation for the reaction between Al and O2 is:
4 Al + 3 O2 → 2 Al2O3
According to the equation, 4 moles of Al react with 3 moles of O2 to produce 2 moles of Al2O3.
Since we have 4.00 moles of Al, we need to determine the mole ratio between Al and O2. By comparing the coefficients in the balanced equation, we can see that the ratio of moles of Al to O2 is 4:3.
To calculate the number of moles of O2 needed, we can use the following proportion:
4.00 moles Al / 4 moles Al : x moles O2 / 3 moles O2
Simplifying the proportion:
(4 moles Al * x moles O2) = (4.00 moles Al * 3 moles O2)
x = (4.00 moles Al * 3 moles O2) / 4 moles Al
Calculating the value:
x = 3.00 moles O2
Therefore, 3.00 moles of O2 are needed for a complete reaction with 4.00 moles of Al.