Question

How many liters of H2S at STP will react with 27.8 g of oxygen to form sulfur dioxide and water? 2H2S + 3O2 --> 2SO2 + 2H2O

Answer 1

12.973 liters of H2S is required at STP.

Step-by-step explanation:

The given equation is ,

2H2S + 3O2 --> 2SO2 + 2H2O , mass of reacting O2 is 27.8 g

The mole ratio is,

`(H2S)/(O2) = (2)/(3)`

number of moles = m =
`(mass of substance)/(molecular weight of compound)`

for O2, m =
`(27.8)/(32)` (molecular weight of O2 is 32)

number of moles of H2S is

`((2)/(3))((27.8)/(32))`

now at STP, 1 mole of gas occupies 22.4 liters.

thus liters of H2S required are,

`((2)/(3))((27.8)/(32))(22.4)` = 12.973 liters