Answer:
- 1. Iodine is the limiting reactant
Explanation:
1. Balanced chemcial equation:
[tex]2Al+3I_2\rightarrow 2AlI_3[/tex]
2. Theoretical mole ratio
It is the ratio of the coefficients of the reactants in the balanced chemical equation:
[tex]\dfrac{2molAl}{3molI_2}[/tex]
3. Actual ratio
It is ratio of the moles available to reat:
[tex]\dfrac{9molAl}{9molI_2}[/tex]
4. Comparison
[tex]\dfrac{9molAl}{9molI_2}>\dfrac{2molAl}{3molI_2}[/tex]
Then, there are more aluminum available than what is needed to react with the 9 moles of iodine, meaning that the aluminum is in excess and the iodine will react completely, being the latter the limiting reactant.
Conclusion: iodine is the limiting reactant.
5. How much aluminum iodide will be produced?
Use the theoretical mole ratio of aluminum iodide to iodide:
[tex]\dfrac{2molAlI_3}{3molI_2}\times 9molI_2=6molAlI_3\leftarrow answer[/tex]
