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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
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To solve this problem, we need to follow these steps:1. Write the balanced chemical equation for the reaction between barium oxide (BaO) and sulfuric acid (H2SO4).2. Calculate the molar mass of H2SO4.3. Convert the given mass of H2SO4 to moles.4. Use the stoichiometry of the reaction to determine the moles of water (H2O) produced.5. Convert the moles of water to liters.Step 1: Balanced chemical equationBaO + H2SO4 → BaSO4 + H2OStep 2: Molar mass of H2SO4Molar mass of H2SO4 = 2(1.01) + 32.07 + 4(16.00) = 98.09 g/molStep 3: Convert the given mass of H2SO4 to molesMoles of H2SO4 = 183.3 g / 98.09 g/mol = 1.87 molStep 4: Use the stoichiometry of the reactionAccording to the balanced equation, 1 mole of H2SO4 produces 1 mole of H2O.Moles of H2O = 1.87 molStep 5: Convert the moles of water to litersAt standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters.Liters of H2O = 1.87 mol × 22.4 L/mol = 41.9 LTherefore, 41.9 liters of water can be formed from 183.3 g of H2SO4.