Question

What are the correct coefficients when this equation is balanced?

Answer 1

Answer:

4 Sb, 3 $O_{2}$

Explanation:

  On the reactant's side of the equation (the left side), there is one Antimony and one Oxygen gas molecule ($O_{2}$). The oxygen gas molecule is made of two atoms, so we actually have 2 oxygens on the left side. On the product's side (the right side), there are 4 antimony atoms, and 6 oxygen atoms. If we were to write it out in a certain way, it would look like this:

__Sb + __ $O_{2}$ --> $Sb_{4} O_{6}$

                  1   Sb   4

                  2   O   6

  To balance this equation, those numbers on either side of the elements must equal each other. We can accomplish this with the proper coefficients. If we put a 4 in front of the antimony, it means this:

4 Sb + __ $O_{2}$ --> $Sb_{4} O_{6}$

                  4   Sb   4

                  2   O   6

And the antimony is now balanced.

  Now we must balance the oxygen. There are 6 oxygens on the product's side but only 2 on the reactant's side. To fix this, simply multiply the oxygen by 3:

4 Sb + 3 $O_{2}$ --> $Sb_{4} O_{6}$

              4   Sb   4

              6   O   6

3 * 2 = 6, so now oxygen is balanced, and the equation is now correct.