Question

0.5 mole of H₂S and SO₂ are mixed together in a reaction flask in which the following reaction tales place–

2H₂S(g) + SO₂(g) → 2H₂O(l) + 3S(s)

Calculate the number of moles of Sulphur formed.

Answer 1

2H₂S(g) + SO₂(g) → 2H₂O(l) + 3S(s)

\(\because\) 2 moles of H₂S react with 1 mol of SO₂

to produce = 3 moles of Sulphur

\(\therefore\) 0.5 mol H₂S will react with 0.25 mol SO₂

to produce = \(\frac{3}{2}\) x 0.5

= 0.75 mol of sulphur