Question

What mass of oxgyen is need to react with 8.5g of hydrogen sulphide(H₂S)?

2 H₂S + 3 O₂ -> 2 SO₂ + 2 H₂O

Answer 1

To react completely with 8.5 g of hydrogen sulfide, approximately 11.97 g of oxygen is needed, as determined through stoichiometric calculations based on the balanced chemical equation.

Step-by-step explanation:

Stoichiometry Calculation for Oxygen and Hydrogen Sulfide Reaction:

To determine the mass of oxygen needed to react with hydrogen sulfide (H₂S), we should use the stoichiometry of the balanced chemical equation:

2 H₂S (g) + 3 O₂ (g) → 2 SO₂ (g) + 2 H₂O (g)

First, we calculate the molar mass of H₂S which is (2×1.008) + 32.07 = 34.08 g/mol. Then, using the mass of hydrogen sulfide provided (8.5 g), we find the number of moles of H₂S:

1. Moles of H₂S = mass of H₂S / molar mass of H₂S = 8.5 g / 34.08 g/mol = 0.249 mol.
2. According to the balanced equation, 2 moles of H₂S react with 3 moles of O₂. Therefore, 0.249 moles of H₂S will need 0.249 mol × (3 moles O₂ / 2 moles H₂S) = 0.374 mol of O₂.
3. The molar mass of O₂ is 32.00 g/mol. So, the mass of O₂ required is 0.374 mol × 32.00 g/mol = 11.97 g of O₂.

We conclude that approximately 11.97 g of oxygen is needed to completely react with 8.5 g of hydrogen sulfide.

Answer 2

To react with 8.5 g of hydrogen sulfide, 12.00 g of oxygen is needed based on stoichiometric calculations from the balanced chemical equation.

Step-by-step explanation:

To calculate the mass of oxygen needed to react with 8.5g of hydrogen sulfide (H2S), we use the balanced chemical equation: 2H2S (g) + 3O2 (g) → 2SO2 (g) + 2H2O(g).

First, we find the molar mass of H2S, which is approximately 34.08 g/mol. Next, we calculate the number of moles of H2S in 8.5 g:

Moles of H2S = 8.5 g / 34.08 g/mol

≈ 0.25 moles.

According to the balanced equation, 2 moles of H2S react with 3 moles of O2. Therefore, the moles of O2 needed will be:

Moles of O2 = (3 moles O2 / 2 moles H2S) × 0.25 moles H2S

= 0.375 moles O2.

The molar mass of O2 is 32.00 g/mol, so the mass of O2 required is:

Mass of O2 = 0.375 moles × 32.00 g/mol

= 12.00 g.

So, 12.00 g of oxygen is needed to react with 8.5 g of hydrogen sulfide.