Question

Balance the equation :

Answer 1

The balanced equation is 2 AlI 3 ( a q ) + 3 Cl 2 ( g ) → 2 AlCl 3 ( a q ) + 3 I 2 ( g ) .

Explanation:

• Aluminum has a typical oxidation condition of  3+  , and that of iodine is  1-  .   Along these lines, three iodides can bond with one aluminum. You get  AlI3.  For comparable reasons, aluminum chloride is  AlCl3.  

• Chlorine and iodine both exist normally as diatomic components, so they are  Cl2(  g  )  also,  I2(  g  ), individually. In spite of the fact that I would anticipate that iodine should be a strong.  

Balancing the equation, we get:  

            2AlI 3(  aq  )  +  3Cl2 (  g  )  →  2AlCl3 (  aq  )   +  3 I 2  (  g  )  

• Realizing that there were two chlorines on the left, I simply found the basic numerous of 2 and 3 to be 6, and multiplied the  AlCl  3  on the right.  

• Normally, presently we have two  Al  on the right, so I multiplied the  AlI  3  on the left. Hence, I have 6  I  on the left, and I needed to significantly increase  I 2  on the right.  

• We should note, however, that aluminum iodide is viciously receptive in water except if it's a hexahydrate. In this way, it's most likely the anhydrous adaptation broke down in water, and the measure of warmth created may clarify why iodine is a vaporous item, and not a strong.