Given the equation 2H_(2)Oarrow 2H_(2)+O_(2) how many moles of H_(2)O would be required to produce 80 g of O_(2) A. 1.0 mol B. 2.0 mol C. 4.0 mol D. 5.0 mol A B c D

To solve this problem, we need to use the concept of stoichiometry and the molar mass of oxygen (O2).<br /><br />Given information:<br />- The balanced chemical equation is: 2H2O → 2H2 + O2<br />- We need to find the number of moles of H2O required to produce 80 g of O2.<br /><br />Step 1: Calculate the molar mass of O2.<br />Molar mass of O2 = 16.00 g/mol × 2 = 32.00 g/mol<br /><br />Step 2: Calculate the number of moles of O2.<br />Number of moles of O2 = 80 g / 32.00 g/mol = 2.5 mol<br /><br />Step 3: Use the stoichiometric relationship between H2O and O2.<br />According to the balanced equation, 2 moles of H2O are required to produce 1 mole of O2.<br />Therefore, the number of moles of H2O required = 2 × 2.5 mol = 5.0 mol<br /><br />Therefore, the correct answer is D. 5.0 mol.