If you produce 3.5 moles of H2, how many moles of aluminum did you use in the reaction?
What reaction?
The reaction is 2Al+2NaOH+4H2O==> 2NaAl(OH)4+H2
To determine the number of moles of aluminum used in the reaction, we need to know the balanced chemical equation for the reaction between aluminum and hydrogen gas. This equation will give us the stoichiometric relationship between the two compounds.
Assuming the balanced chemical equation for the reaction is:
2Al + 3H2 -> 2AlH3
In this equation, it states that 2 moles of aluminum react with 3 moles of hydrogen gas to produce 2 moles of aluminum hydride.
Now, we know that we produced 3.5 moles of H2. By using the molar ratio from the balanced equation, we can determine the moles of aluminum used in the reaction.
From the equation, we see that 3 moles of H2 react with 2 moles of aluminum. Therefore, the moles of aluminum used can be calculated using the following proportion:
(2 moles Al / 3 moles H2) = (x moles Al / 3.5 moles H2)
Simplifying the proportion, we find:
x moles Al = (2 moles Al / 3 moles H2) * 3.5 moles H2
x moles Al = 2.33 moles Al
Therefore, you would have used approximately 2.33 moles of aluminum in the reaction.