Formula 1 point When barium oxide and sulfuric acid (H_(2)SO_(4)) are combined, barium sulfate and water are formed. underline ( )BaO+underline ( )H_(2)SO_(4)arrow underline ( )BaSO_(4)+underline ( )H_(2)O How many liters of water can be formed from 183.3 g of H_(2)SO_(4) Type square

To solve this problem, we need to follow these steps:<br /><br />1. Write the balanced chemical equation for the reaction between barium oxide (BaO) and sulfuric acid (H2SO4).<br />2. Calculate the molar mass of H2SO4.<br />3. Convert the given mass of H2SO4 to moles.<br />4. Use the stoichiometry of the reaction to determine the moles of water (H2O) produced.<br />5. Convert the moles of water to liters.<br /><br />Step 1: Balanced chemical equation<br />BaO + H2SO4 → BaSO4 + H2O<br /><br />Step 2: Molar mass of H2SO4<br />Molar mass of H2SO4 = 2(1.01) + 32.07 + 4(16.00) = 98.09 g/mol<br /><br />Step 3: Convert the given mass of H2SO4 to moles<br />Moles of H2SO4 = 183.3 g / 98.09 g/mol = 1.87 mol<br /><br />Step 4: Use the stoichiometry of the reaction<br />According to the balanced equation, 1 mole of H2SO4 produces 1 mole of H2O.<br />Moles of H2O = 1.87 mol<br /><br />Step 5: Convert the moles of water to liters<br />At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters.<br />Liters of H2O = 1.87 mol × 22.4 L/mol = 41.9 L<br /><br />Therefore, 41.9 liters of water can be formed from 183.3 g of H2SO4.