How many grams of H₂O will be formed when 32.0 g H₂ is mixed with 12.0 g of O₂ and allowed to react to form water? A)13.5 g B)286 g C)6.8 g D)3.4 g E)144 g

Question

Quizplus · Accepted Answer

The given chemical formulas seem to be incorrectly formatted, but assuming the intention is to describe a reaction between hydrogen sulfide (H2S) and oxygen (O2) to form water (H2O), we can proceed with stoichiometry. The reaction is: 2H2S + 3O2 → 2H2O + 2SO2. From the given masses, we first determine the limiting reactant. The molar mass of H2S is approximately 34.08 g/mol, and for O2, it is about 32.00 g/mol. With 32.0 g of H2S, we have 32.0 g / 34.08 g/mol ≈ 0.939 mol of H2S. For 12.0 g of O2, we have 12.0 g / 32.00 g/mol = 0.375 mol of O2. The stoichiometry of the reaction requires 3 moles of O2 for every 2 moles of H2S. Thus, O2 is the limiting reactant. The amount of H2O produced can be calculated from the amount of O2 reacted. Since 3 moles of O2 produce 2 moles of H2O, 0.375 moles of O2 will produce (0.375 mol O2 * 2 mol H2O / 3 mol O2) = 0.25 mol H2O. The molar mass of H2O is approximately 18.015 g/mol, so the mass of H2O produced is 0.25 mol * 18.015 g/mol = 4.504 g. However, the question seems to contain a misunderstanding or misprint regarding the formation of water and the substances involved. Given the options and assuming a simple stoichiometric calculation was intended, none of the provided answers directly match the calculated result, suggesting a possible error in the interpretation of the question or in the provided options.

How Many Grams of H2O Will Be Formed When 32

How Many Grams of H₂O Will Be Formed When 32