Question

What are the products of Al+MgCl2 and how do I balance it and what type of reaction is it?

Answer 1

his would be a single displacement reaction ,
\[2Al+3MgCl _{2}=2AlCl _{3}+3Mg\] the way you about balancing these equation is first figuring out what type of reaction will take place. In this case we have a single displacement where the chlorine disassociates with the magnesium and then bonds itself to the aluminum.

After you've found what would happen in your reaction, you then need to balance the ionic charges in this case , Al +3 , Cl -1 and Mg +2 . Which gives you the values needed to balance so that the compound will have a net ionic 0 so they will bond. In this case when on the left we have

\[Al ^{+3}+ Mg ^{+2} Cl _{2}^{-1} = Al ^{+3} Cl _{3}^{-1}+Mg ^{+2} \]
For the compound to balance you see that you need 2 chlorine on the left side and 3 chlorine on the right

Lastly you have to balance the equation so there is an equal amount in your reagents(reactants) and products.