Balance this equation: P_(4)+O_(2)... P_(2)O_(3) P_(4)+3O_(2)-gt 2P_(2)O_(3) P_(4)+O_(2)... 2P_(2)O_(3) C P_(4)+2O_(2)arrow 3P_(2)O_(3) 3P_(4)+O_(2)-gt 2P_(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, we have 4 phosphorus atoms on the left side and 2 phosphorus atoms on the right side. To balance the phosphorus atoms, we need to have 2 molecules of $P_{2}O_{3}$ on the right side. This gives us a total of 4 phosphorus atoms on both sides.<br /><br />Next, we need to balance the oxygen atoms. On the left side, we have 2 oxygen atoms from $O_{2}$. On the right side, each molecule of $P_{2}O_{3}$ has 3 oxygen atoms, and we have 2 molecules of $P_{2}O_{3 of 6 oxygen atoms. To balance the oxygen atoms, we need to have 3 molecules of $O_{2}$ on the left side.<br /><br />Therefore, the balanced equation is $P_{4}+3O_{2}\rightarrow 2P_{2}O_{3}$.