Question

The equation for the reaction between hydrogen sulfide, H2S, and oxygen is shown.

2H2S + 302 → 2S02 + 2H20
Which mass of oxygen is required to react with 5.1 g of hydrogen sulfide?

Answer 1

Using stoichiometry, we find that 7.1872 g of oxygen (O2) are required to react with 5.1 g of hydrogen sulfide (H2S) based on the balanced chemical equation.

Step-by-step explanation:

To determine the mass of oxygen required to react with 5.1 g of hydrogen sulfide (H2S), we can use stoichiometry and the balanced chemical equation 2H2S + 3O2 → 2SO2 + 2H2O. First, calculate the number of moles of H2S present in 5.1 g using its molar mass (34.08 g/mol for H2S). Once the moles of H2S are known, use the molar ratio from the balanced equation to find the moles of O2 needed (3 moles O2 for every 2 moles H2S). Finally, convert the moles of oxygen to grams using the molar mass of oxygen (32.00 g/mol for O2).

Here's the calculation process:

1. Calculate moles of H2S: (5.1 g H2S) / (34.08 g/mol) = 0.1497 moles H2S.
2. Calculate moles of O2 needed using mole ratio: (0.1497 moles H2S) × (3 moles O2 / 2 moles H2S) = 0.2246 moles O2.
3. Calculate mass of O2: (0.2246 moles O2) × (32.00 g/mol) = 7.1872 g O2.

Therefore, 7.1872 g of O2 are required to react with 5.1 g of H2S.