Given the equation 2H_(2)Oarrow 2H_(2)+O_(2) how many moles of H_(2)O would be required to produce 2.5 moles of O_(2) A. 1.0 mol B. 2.0 mol C. 4.0 mol D. 5.0 mol A B C D

To determine how many moles of \( H_2O \) are required to produce 2.5 moles of \( O_2 \), we need to use the stoichiometric relationship from the balanced chemical equation:<br /><br />\[ 2H_2O \rightarrow 2H_2 + O_2 \]<br /><br />From the equation, we see that 2 moles of \( H_2O \) produce 1 mole of \( O_2 \). Therefore, the ratio of \( H_2O \) to \( O_2 \) is 2:1.<br /><br />Given that we need to produce 2.5 moles of \( O_2 \), we can set up the proportion:<br /><br />\[ \frac{2 \text{ moles } H_2O}{1 \text{ mole } O_2} = \frac{x \text{ moles } H_2O}{2.5 \text{ moles } O_2} \]<br /><br />Solving for \( x \):<br /><br />\[ x = 2 \times 2.5 = 5 \text{ moles } H_2O \]<br /><br />So, 5.0 moles of \( H_2O \) are required to produce 2.5 moles of \( O_2 \).<br /><br />The correct answer is:<br />D. 5.0 mol