Final answer:
To determine the mass of oxygen required to react with 5.1 g of hydrogen sulfide, first calculate the moles of H2S using its molar mass. Then, use the mole ratio to find the moles of O2 required. Finally, convert the moles of O2 to grams using its molar mass to find the mass of oxygen. Therefore, 3.19 g of oxygen is required to react with 5.1 g of hydrogen sulfide.
Step-by-step explanation:
In the equation 2H2S + O2 → 2H2O + 2SO2, the molar ratio between H2S and O2 is 2:3. To determine the mass of oxygen required to react with 5.1 g of hydrogen sulfide, you can use the concept of stoichiometry. First, calculate the moles of H2S using its molar mass. Then, use the mole ratio to find the moles of O2 required. Finally, convert the moles of O2 to grams using its molar mass to find the mass of oxygen.
Step 1: Calculate moles of H2S using its molar mass:
Mass of H2S = 5.1 g
Molar mass of H2S = 34.08 g/mol (2 * 1.01 g/mol for hydrogen + 32.07 g/mol for sulfur)
Moles of H2S = Mass of H2S / Molar mass of H2S
Step 2: Use the mole ratio between H2S and O2 to find moles of O2 required:
Mole ratio between H2S and O2 = 2/3
Moles of O2 = Moles of H2S * (2/3)
Step 3: Convert moles of O2 to grams:
Molar mass of O2 = 32.00 g/mol (16.00 g/mol per oxygen atom * 2 oxygen atoms)
Mass of O2 = Moles of O2 * Molar mass of O2
Substitute the values into the equations and calculate the result:
Mass of H2S = 5.1 g / 34.08 g/mol = 0.1497 mol
Moles of O2 = 0.1497 mol * (2/3) = 0.0998 mol
Mass of O2 = 0.0998 mol * 32.00 g/mol = 3.19 g
Therefore, 3.19 g of oxygen is required to react with 5.1 g of hydrogen sulfide.