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

Partial pressure of hydrogen gas
`V_(1)=0.5L" "V_(2)=1L`
`p_(1)="0.8 bar "p_(2)=?`
Applying Boyle.s law (constant T and n)
`p_(1)V_(1)=p_(2)V_(2)" or "p_(2)=(p_(1)V_(1))/(V_(2))`
`therefore" "p_(2)=(("0.8 bar")xx(0.5 L))/(1L)`
`="0.40 bar"`
Partial pressure of oxygen gas,
`V_(1)=2.0L," "V_(2)=1.0L`
`p_(1)="0.7 bar "p_(2)=?`
`"or "p_(2)=(p_(1)V_(1))/(V_(2))=(("0.7 bar")xx(2.0L))/((1.0L))="1.40 bar"`
Pressure of the gas mixture,
`p_("mix")=p_(H_(2))+p_(O_(2))`
`=0.40+1.40="1.80 bar."`