P_(4)+3O_(2)arrow P_(4)O_(6) What is the limiting reactant is 12 moles of P_(4) react with 15 moles of O_(2) P_(4)= P_(4)O_(6) O_(2) none of the above

To determine the limiting reactant, we need to compare the mole ratio of the reactants with the stoichiometric ratio in the balanced chemical equation.<br /><br />The balanced chemical equation is:<br />$P_{4} + 3O_{2} \rightarrow P_{4}O_{6}$<br /><br />From the equation, we can see that 1 mole of $P_{4}$ reacts with 3 moles of $O_{2}$ to produce 1 mole of $P_{4}O_{6}$.<br /><br />Given that we have 12 moles of $P_{4}$ and 15 moles of $O_{2}$, we can calculate the required moles of $O_{2}$ for 12 moles of $P_{4}$ to react completely:<br />Required moles of $O_{2}$ = 12 moles of $P_{4} \times 3 = 36$ moles of $O_{2}$<br /><br />Since we only have 15 moles of $O_{2}$, which is less than the required 36 moles, $O_{2}$ is the limiting reactant.<br /><br />Therefore, the correct answer is:<br />$O_{2}$