How do you balance #Al+Cl_2->AlCl_3#?
1 Answer
Explanation:
Let's balance this equation by using oxidation numbers.
Start by assigning oxidation numbers to the atoms that take part in the reaction
#stackrel(color(blue)(0))("Al") _ ((s)) + stackrel(color(blue)(0))("Cl")_ (2(g)) -> stackrel(color(blue)(+3))("Al") stackrel(color(blue)(-1))("Cl")_ (3(s))#
Notice that the oxidation number of aluminium increases from
On the other hand, the oxidation number of chlorine decreases from
The oxidation half-reaction looks like this
#stackrel(color(blue)(0))("Al") -> stackrel(color(blue)(+3))("Al")""^(3+) + 3"e"^(-)#
The reduction half-reaction looks like this
#stackrel(color(blue)(0))("Cl")_ 2 + "e"^(-) -> stackrel(color(blue)(-1))("Cl")""^(-)#
Balance the chlorine atoms by multiplying the product by
#stackrel(color(blue)(0))("Cl")_ 2 + 2"e"^(-) -> 2stackrel(color(blue)(-1))("Cl")""^(-)#
Now, in any redox reaction, the number of electrons lost in the oxidation half-reaction must be equal to the number of electrons gained in the reduction half-reaction.
To get them to balance out, multiply the oxidation half-reaction by
#{(color(white)(aaaaaa)stackrel(color(blue)(0))("Al") -> stackrel(color(blue)(+3))("Al")""^(3+) + 3"e"^(-)" "| xx 2), (stackrel(color(blue)(0))("Cl")_ 2 + 2"e"^(-) -> 2stackrel(color(blue)(-1))("Cl")""^(-)" "color(white)(aaaaa)| xx 3) :}#
#color(white)(a)/color(white)(aaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaaa)#
#2"Al" + 3"Cl"_ 2 + color(red)(cancel(color(black)(6"e"^(-)))) -> 2"Al"^(3+) + 6"Cl"^(-) + color(red)(cancel(color(black)(6"e"^(-))))#
This will be equivalent to
#2"Al" + 3"Cl"_ 2 -> 2 xx ["Al"^(3+) + 3"Cl"^(-)]#
which of course gets you
#color(green)(|bar(ul(color(white)(a/a)color(black)(2"Al"_ ((s)) + 3"Cl"_ (2(g)) -> 2"AlCl"_ (3(s)))color(white)(a/a)|)))#