Passing an electric current through a sample of water (H2O) can cause the water to decompose into hydrogen gas (H2) and oxygen g
as (O2) according to the following equation. 2H2O mc026-1.jpg 2H2 + O2 The molar mass of H2O is 18.01 g/mol. The molar mass of O2 is 32.00 g/mol. What mass of H2O, in grams, must react to produce 50.00 g of O2? 14.07 23.05 28.14 56.28
2H2O --> 2H2 + O2 The mole H2O:mole O2 ratio is 2:1 Now determine how many moles of O2 are in 50g: 50g × 1mol/32g = 1.56 moles O2 Since 1 mole of O2 was produced for every 2 moles of H2O, we need 2×O2moles = H2O moles 2×1.56 = 3.13 moles H2O Finally, convert moles to grams for H2O: 3.13moles × 18g/mol = 56.28 g H2O D) 56.28
