What will be the pressure of the gas mixture when `0.5 L` of `H_(2)` at `0.8` bar `2.0 L` of oxygen at `0.7` bar are introduced in a `1L` vessel at `27^(@)C` ?

Explanation

Step I:
To calculate the particle pressure of hydrogen
`V_(1)=0.5 L," " V_(2)=1 L`
`P_(1)=0.8 "bar", " "P_(2)=?`
Applying Boyle's law
`P_(1)V_(1)=P_(2)V_(2)`
`0.8xx0.5=P_(2)xx1` or `P_(2)=0.40 "bar"`
Step II:
To calculate the particle pressure of oxygen
`V_(1)=2.0 L, " "V_(2)=1 L`
`P_(1)=0.7 "bar"," " P_(2)=?`
Applying Boyle's law
`P_(1)V_(1)=P_(2)V_(2)`
`0.7xx2=P_(2)xx1` or `P_(2)=1.4 "bar"`
Step III:
If `P` is the final pressure of the gaseous mixture, then according to Dalton's law of partial pressure
`P=P_(H_(2))+P_(O_(2))=(0.40+1.4) "bar"=1.8 "bar"`