Balance this equation: P_(4)+O_(2)arrow P_(2)O_(3) 3P_(4)+O_(2)arrow 2P_(2)O_(3) P_(4)+O_(2)arrow 2P_(2)O_(3) P_(4)+3O_(2)arrow 2P_(2)O_(3) P_(4)+2O_(2)arrow 3P_(2)O_(3)

The correct balanced equation is:<br />$P_{4}+3O_{2}\rightarrow 2P_{2}O_{3}$<br /><br />Explanation:<br />In the given equation, there are 4 phosphorus atoms on the left side and 2 phosphorus atoms on the right side. To balance the phosphorus atoms, we need to multiply the number of $P_{2}O_{3}$ molecules on the right side by 2, resulting in 4 phosphorus atoms on both sides.<br /><br />Next, we need to balance the oxygen atoms. On the left side, there are 2 oxygen atoms in $O_{2}$, and on the right side, there are 3 oxygen atoms in $P_{2}O_{3}$. To balance the oxygen atoms, we need to multiply the number of $O_{2}$ molecules on the left side by 3, resulting in 6 oxygen atoms on both sides.<br /><br />Therefore, the balanced equation is $P_{4}+3O_{2}\rightarrow 2P_{2}O_{3}$.