Answer:
physcial change
Explanation:
As it has visible changes on shape and size
<u>Answer:</u> The correct answer is Option D.
<u>Explanation:</u>
To calculate the hybridization of
, we use the equation:
![\text{Number of electron pair}=\frac{1}{2}[V+N-C+A]](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20electron%20pair%7D%3D%5Cfrac%7B1%7D%7B2%7D%5BV%2BN-C%2BA%5D)
where,
V = number of valence electrons present in central atom (S) = 6
N = number of monovalent atoms bonded to central atom = 0
C = charge of cation = 0
A = charge of anion = 0
Putting values in above equation, we get:
![\text{Number of electron pair}=\frac{1}{2}[6]=3](https://tex.z-dn.net/?f=%5Ctext%7BNumber%20of%20electron%20pair%7D%3D%5Cfrac%7B1%7D%7B2%7D%5B6%5D%3D3)
The number of electron pair around the central metal atom are 3. This means that the hybridization will be
and the electronic geometry of the molecule will be trigonal planar.
Hence, the correct answer is Option D.
Answer:
- 1. Iodine is the limiting reactant
- 2.

Explanation:
<u>1. Balanced chemcial equation:</u>

<u>2. Theoretical mole ratio</u>
It is the ratio of the coefficients of the reactants in the balanced chemical equation:

<u>3. Actual ratio</u>
<u />
It is ratio of the moles available to reat:

<u>4. Comparison</u>

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.
<u>5. How much aluminum iodide will be produced?</u>
Use the theoretical mole ratio of aluminum iodide to iodide:
