Calculate

the

theoretical

yield

in

grams AlI₃

from

the

complete

reaction

of

113

grams I₂

according

to

the

following

balanced

chemical

equation:

2

Al(s)

+

3

I₂(s)

→

2

AlI₃(s)

To calculate the theoretical yield of aluminum iodide (AlI₃) from a reaction involving iodine (I₂), we need to follow these steps:

### Given Information:
- Mass of I₂ = 113 grams
- Balanced chemical equation:  
  \[
  2\text{Al}(s) + 3\text{I}_2(s) \rightarrow 2\text{AlI}_3(s)
  \]

### Step 1: Calculate the molar mass of I₂ and AlI₃.
- Iodine (I) has an atomic mass of approximately 126.90 g/mol, so:
  \[
  \text{Molar mass of I}_2 = 2 \times 126.90 \, \text{g/mol} = 253.80 \, \text{g/mol}
  \]
  
- The molar mass of AlI₃ is calculated by summing the atomic masses of aluminum (Al) and iodine (I):
  \[
  \text{Molar mass of AlI}_3 = \text{Al} + 3 \times \text{I} = 26.98 \, \text{g/mol} + 3 \times 126.90 \, \text{g/mol} = 407.68 \, \text{g/mol}
  \]

### Step 2: Convert the mass of I₂ to moles.
Use the molar mass of I₂ to find the moles of iodine:
\[
\text{Moles of I}_2 = \frac{\text{Mass of I}_2}{\text{Molar mass of I}_2} = \frac{113 \, \text{g}}{253.80 \, \text{g/mol}} = 0.445 \, \text{mol}
\]

### Step 3: Use the stoichiometric ratio from the balanced equation.
From the balanced equation, the mole ratio between I₂ and AlI₃ is 3:2, meaning that 3 moles of I₂ produce 2 moles of AlI₃.

\[
\text{Moles of AlI}_3 = \left( \frac{2 \, \text{mol AlI}_3}{3 \, \text{mol I}_2} \right) \times 0.445 \, \text{mol I}_2 = 0.297 \, \text{mol AlI}_3
\]

### Step 4: Convert moles of AlI₃ to grams.
Now, we use the molar mass of AlI₃ to convert the moles of AlI₃ to grams:
\[
\text{Mass of AlI}_3 = 0.297 \, \text{mol} \times 407.68 \, \text{g/mol} = 121.12 \, \text{g}
\]

### Theoretical Yield:
The theoretical yield of AlI₃ is approximately **121.12 grams**.

Would you like more details or have any questions?

Here are five related questions:
1. How do you calculate the molar mass of compounds in complex reactions?
2. What is the importance of the stoichiometric ratio in determining yields?
3. How does the limiting reagent affect the theoretical yield?
4. Can the actual yield exceed the theoretical yield in a chemical reaction?
5. What factors might cause the theoretical yield to not match the actual yield?

**Tip**: Always check if you have the limiting reagent before calculating yields!

Calculate the theoretical yield in grams AlI₃ from the complete reaction of 113 grams I₂ according to the following balanced chemical equation: 2Al(s) + 3I₂(s) → 2AlI₃(s)

Learn how to calculate the theoretical yield of aluminum iodide (AlI₃) from 113 grams of iodine (I₂) using stoichiometry. This problem involves mole conversions, mass-to-mole calculations, and the use of stoichiometric ratios. Perfect for high school chemistry students in Grades 10-12.

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