Question

10.Calculate the volume of oxygen that reacts with 500cm3 of hydrogen sulfide with the volume of both gases measured at rtp:

2H2S + 3O2 ------> 2SO2 + 2H20

Answer 1

0.79dm³

Step-by-step explanation:

The reaction expression is given as:

2H₂S + 3O₂ → 2SO₂ + 2H₂O

Volume of hydrogen sulfide = 500cm³ = 0.5dm³

Unknown:

volume of oxygen that reacted = ?

Solution:

At rtp;

22.4dm³ of gas has a mole of 1

0.5dm³ will
`(0.5)/(22.4)` = 0.022mole of hydrogen sulfide;

2 mole of H₂S combines with 3 mole of O₂

0.022 mole of H₂S will combine with
`(0.022 x 3)/(2)` = 0.033mole of O₂

So;

Since;

1 mole of a gas occupied a volume of 22.4dm³ at rtp;

0.033mole of Oxygen gas will occupy 0.033 x 22.4 = 0.79dm³