The balanced chemical equation for the reaction of H2SO4 with water (H2O) is:
H2SO4 + H2O → H3O+ + HSO4-
From this equation, we can see that 1 mole of H2SO4 reacts with 1 mole of water to produce 1 mole of H3O+ and 1 mole of HSO4-. The molar mass of H2SO4 is 98.079 g/mol. Therefore, we can calculate the number of moles of H2SO4 present in 96.0 grams by dividing the mass by the molar mass:
Number of moles of H2SO4 = 96.0 g / 98.079 g/mol = 0.9795 mol
Since the reaction is 1:1 between H2SO4 and H2O, we can see that 0.9795 moles of H2O will be formed as well. The molar mass of H2O is 18.015 g/mol, so we can calculate the mass of H2O formed by multiplying the number of moles by the molar mass:
Mass of H2O formed = 0.9795 mol * 18.015 g/mol = 17.644 g
Therefore, 96.0 grams of H2SO4 can produce 17.644 grams (or 17.644 mL, assuming standard temperature and pressure) of H2O. Rounded to three decimal places, the answer is 17.644 g.