Question

1. A mixture contains 8.00 g each of O2, CO2, and SO2 at STP. Calculate the volume of this mixture. Which of the gases would exert the greatest pressure and why?

Answer 1

Step-by-step explanation:

mole of O₂ =
`(8)/(32)`

= .25 moles

mole of CO₂

=
`(8)/(44)`

= .1818 moles

moles of SO₂

`(8)/(64)`

= .125 moles

Total moles of gas

= .5568 moles.

total volume of gas mixture

= 22.4 x .5568 liter ( volume of one mole of any gas = 22.4 liter)

= 12.47 liter.

gas will exert partial pressure according to their mole fraction

gas having greatest no of moles in the total mole will have greatest mole fraction so

O₂ will have greatest partial pressure.