Question

What are the correct coefficients when this equation is balanced?

___ Sb + __ O2 --> Sb4O6

Answer 1

4 Sb, 3
`O_(2)`

Step-by-step 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.